Lecture Presentation
Chapter 2
Atoms, Molecules,
and Ions
© 2015 Pearson Education, Inc.
James F. Kirby
Quinnipiac University
Hamden, CT
Atomic Theory of Matter
The theory that atoms
are the fundamental
building blocks of
matter reemerged in the
early nineteenth
century, championed by
John Dalton.
Atoms,
Molecules,
and Ions
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Dalton’s Postulates
1) Each element is
composed of
extremely small
particles called
atoms.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Dalton’s Postulates
2) All atoms of a given
element are identical
to one another in
mass and other
properties, but the
atoms of one element
are different from the
atoms of all other
elements.
Atoms,
Molecules,
and Ions
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Dalton’s Postulates
3) Atoms of an element
are not changed into
atoms of a different
element by chemical
reactions; atoms are
neither created nor
destroyed in chemical
reactions.
Atoms,
Molecules,
and Ions
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Law of Conservation of Mass
 The total mass of substances present at the
end of a chemical process is the same as the
mass of substances present before the
process took place.
 This law was one of the laws on which
Dalton’s atomic theory was based.
 Lavoisier
Atoms,
Molecules,
and Ions
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Dalton’s Postulates
4) Atoms of more than
one element combine
to form compounds;
a given compound
always has the same
relative number and
kind of atoms.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
My fourt posulate is an extension of a law formulated by the
French chemist, Joseph Proust (1754-1826), in 1799. Proust’s
Law of Definite Proportions states:
Different samples of the same compound always contain its constituent elements in the same proportion by mass.
If we analyzed any number of samples of sodium chloride, NaCl,
collected from different sources, we would find in each and every
sample the same ratio BY MASS of sodium (Na) to chlorine (Cl).
Thus, if the ratio of the MASSES of different elements in a compound
is fixed, the ratio of the ATOMS of these elements in the compound
must also be constant.
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Atoms,
Molecules,
and Ions
Law of Multiple Proportions
If two elements, A and B, form more
than one compound, the masses of B
that combine with a given mass of A are
in the ratio of small whole numbers.
Dalton predicted this law and observed
it while developing his atomic theory.
When two or more compounds exist
from the same elements, they can
not have the same relative number
Atoms,
Molecules,
of atoms.
and Ions
© 2015 Pearson Education, Inc.
Discovery of Subatomic Particles
• In Dalton’s view, the atom was the
smallest particle possible. Many
discoveries led to the fact that the atom
itself was made up of smaller particles.
Electrons and cathode rays
Radioactivity
Nucleus, protons, and neutrons
Atoms,
Molecules,
and Ions
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ATOMIC STRUCTURE
Dalton thought of atoms as being
indivisible and, thus, extremely small.
Rutherford
WHAT ARE THEY?
SAY IT ISN’T SO!!!
A series of investigations that began
in the 1850s and extended into the
20th century demonstrated clearly
that atoms themselves had internal
structure; i.e., atoms are made up of
even smaller particles!!.
Atoms,
Becquerel
Thomson
Millikan
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Molecules,
and Ions
The Electron (Cathode Rays)
• Streams of negatively charged particles were found to
emanate from cathode tubes, causing fluorescence.
• J. J. Thomson is credited with their discovery (1897).
Atoms,
Molecules,
and Ions
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How do we deduce from the figure that cathode
rays travel from cathode to anode?
a. The cathode and anode are labeled in figure (a).
b. A green gas exists in the vacuum tube.
c. Cathode rays consist of charge particles.
d. the manner in which the magnet diverts the path in
figure (b)
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How do we deduce from the figure that cathode
rays travel from cathode to anode?
a. The cathode and anode are labeled in figure (a).
b. A green gas exists in the vacuum tube.
c. Cathode rays consist of charge particles.
d. the manner in which the magnet diverts the path in
figure (b)
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-
Fluorescent
screen
Anode
Cathode
A
B
High
Voltage
+
Cathode ray tube
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Education,
See©Textbook
page
30 Inc.
In the absence of an
electric field,
electrons emitted by
the cathode are
drawn to the anode,
pass through the
hole in the anode
center, and strike the
fluorescent screen at
point A.
In the presence of an
external electric field,
electrons emitted by the
cathode eventually
strike the fluorescent
screen at point B. This
is due to the negatively
charged electrons being
deflected by the
Atoms,
negative part ofMolecules,
the
electric field andand Ions
attracted toward the
The Electron
Thomson measured the charge/mass ratio of
the electron to be 1.76  108 coulombs/gram
(C/g).
Atoms,
Molecules,
and Ions
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If no magnetic field were applied, would you
expect the electron beam to be deflected upward
or downward by the electric field?
a. Downward because a negative particle is repelled by
a negative plate and attracted to a positive plate.
b. Upward because a negative particle is attracted to a
negative plate and repelled by a positive plate.
c. Downward because a negative particle is attracted to a
negative plate and repelled by a positive plate.
d. Upward because a negative particle is repelled by a
negative plate and attracted to a positive plate.
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If no magnetic field were applied, would you
expect the electron beam to be deflected upward
or downward by the electric field?
a. Downward because a negative particle is repelled by
a negative plate and attracted to a positive plate.
b. Upward because a negative particle is attracted to a
negative plate and repelled by a positive plate.
c. Downward because a negative particle is attracted to a
negative plate and repelled by a positive plate.
d. Upward because a negative particle is repelled by a
negative plate and attracted to a positive plate.
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Using a cathode ray tube and his extensive knowledge
of electromagnetic theory, Thomson determined the
ratio of electric charge to mass for an electron.
-1.76 x 108 coulombs/gram
9.10 x 10-28 g
The coulomb (C) is a
unit of electric charge.
(mass of an
Incredibly individual electron)
small charge
and mass!!
-1.6022 x 10-19 C
(charge on an individual electron)
R. A. Millikan successfully measured the charge on,
and mass of, an individual electron by studying the
motion of single tiny oil drops that acquired charge
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Inc.
from
ions in the air.
QUICK TIME VIDEO
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Robert Millikan’s (in)famous “Oil Drop” Experiment
charge
-1.6022 x 10-19 C
mass of electron = ----------------- = ----------------------- = 9.10 x 10-28 g
charge/mass
-1.76 x 108 C/g
charged
plate
oil droplets
+
+
small
hole
oil droplets
under
observatio
n
atomize
r
charged
plate
© 2015
Education,
(Based
on Pearson
Fig. 2.5,
p. 39,Inc.
Chang 7th ed.)
viewing
microscop
e
Millikan Oil-Drop Experiment
(Electrons)
 Once the charge/mass
ratio of the electron was
known, determination of
either the charge or the
mass of an electron
would yield the other.
 Robert Millikan
determined the charge
on the electron in 1909.
Atoms,
Molecules,
and Ions
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Would the masses of the oil drops be changed
significantly by any electrons that accumulate
on them?
a. Yes, the electrons add significant mass to the oil drop.
b. No, the electrons add only a small mass to the oil drop.
c. Yes, the electrons cause the oil drops to stick together.
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Would the masses of the oil drops be changed
significantly by any electrons that accumulate
on them?
a. Yes, the electrons add significant mass to the oil drop.
b. No, the electrons add only a small mass to the oil drop.
c. Yes, the electrons cause the oil drops to stick together.
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Radioactivity
• Radioactivity is the spontaneous emission of
high-energy radiation by an atom.
• It was first observed by Henri Becquerel.
• Marie and Pierre Curie also studied it.
• Its discovery showed that the atom had more
subatomic particles and energy associated
with it.
Atoms,
Molecules,
and Ions
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Radioactivity
• Three types of radiation were discovered by
Ernest Rutherford:
  particles (positively charged)
  particles (negatively charged, like electrons)
  rays (uncharged)
Atoms,
Molecules,
and Ions
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(1) Which of the three kinds of radiation shown
consists of electrons?
(1)
a. β
b. γ
c. α
d. (A) and (C)
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(1) Which of the three kinds of radiation shown
consists of electrons?
(1)
a. β
b. γ
c. α
d. (A) and (C)
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(2) Why are these rays deflected to a greater
extent than the others?
(2)
a. Beta particles are negatively charged.
b. Alpha particles are positively charged.
c. Alpha particles are less massive than beta particles.
d. Beta particles are less massive than alpha particles.
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(2) Why are these rays deflected to a greater
extent than the others?
(2)
a. Beta particles are negatively charged.
b. Alpha particles are positively charged.
c. Alpha particles are less massive than beta particles.
d. Beta particles are less massive than alpha particles.
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The Atom, circa 1900
• The prevailing theory
was that of the “plum
pudding” model, put
forward by Thomson.
• It featured a positive
sphere of matter with
negative electrons
embedded in it.
Atoms,
Molecules,
and Ions
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Discovery of the Nucleus
Ernest
Rutherford shot
 particles at a
thin sheet of
gold foil and
observed the
pattern of scatter
of the particles.
Atoms,
Molecules,
and Ions
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Structure of the Atom: The Proton & Nucleus
Rutherford’s experiment for measuring scattering of 
particles by a thin metal foil:
E. Rutherford
(1871-1937)

Rutherford used  particles to probe atomic structure.

Thin gold and other metal foils served as targets for 
particles. See the illustration below (from S. Zumdahl slides).

Most of the  particles penetrated the metal foils with little or
no deflection. However, an  particle would be deflected at a
large angle or back toward the source!
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
QUICK TIME
VIDEO
(1908 Nobel Prize in Chemistry)
 particle velocity ~ 1.4 x 107 m/s
(~5% speed of light)
1. atoms positive charge is concentrated in the nucleus
2. proton (p) has opposite (+) charge of electron
Atoms,
-24
Molecules,
3. mass of p is 1840 x mass of e (1.67 x 10 g)
and Ions
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Structure of the Atom: The Proton & Nucleus
Rutherford formulated his model of the atom, based on
the results of his -scattering experiments:

E. Rutherford
(1871-1937)

Mostly empty space, which would explain why most 
particles passed through the foil undetected.
Atom’s positive charges concentrated in the nucleus, a dense
central core within the atom. This would explain why those 
particles that came near or directly at the nucleus experienced
large deflections or reversed directions (repulsion of positive
charge by positive charge).
We now know these positively charged particles in the
nucleus as protons:

Mass of proton = 1.67262 x 10-24 g -- about 1840x the mass of
an electron.

Typical atomic radius is about 100 pm (pm = picometers).
Atoms,
Radius of atomic nucleus ONLY about 5 x 10-3 pm !!! IT’S
Molecules,
LIKE PLACING A MARBLE IN THE MIDDLE OF THE
and Ions
HOUSTON ASTRODOME!!!
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What is the charge on the particles that form
the beam?
a. –1, because the beam consists of beta particles.
b. +2, because the beam consists of alpha particles.
c. +1, because the beam consists of beta particles.
d. –2, because the beam consists of alpha particles.
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What is the charge on the particles that form
the beam?
a. –1, because the beam consists of beta particles.
b. +2, because the beam consists of alpha particles.
c. +1, because the beam consists of beta particles.
d. –2, because the beam consists of alpha particles.
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The Nuclear Atom
Since some particles
were deflected at
large angles,
Thomson’s model
could not be correct.
Atoms,
Molecules,
and Ions
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The Nuclear Atom
• Rutherford postulated a
very small, dense
nucleus with the
electrons around the
outside of the atom.
• Most of the volume is
empty space.
• Atoms are very small;
1 – 5 Å or 100 – 500 pm.
• Other subatomic particles
(protons and neutrons)
were discovered.
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Atoms,
Molecules,
and Ions
What is the approximate diameter of the nucleus
in units of pm?
a. 100 pm
b. 1 pm
c. 10–2 pm
d. 10–4 pm
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What is the approximate diameter of the nucleus
in units of pm?
a. 100 pm
b. 1 pm
c. 10–2 pm
d. 10–4 pm
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Structure of the Atom: The Neutron
Rutherford’s model of the atom left one question unanswered:
Why
is the ratio of
the mass of the He atom to that of the H atom
actually
4:1
We electrons
have very
little mass
compared to
protons!
Thus, our
contribution
to atomic
mass is
negligible!!
instead of the 2:1 ratio
predicted by Rutherford’s
model?
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Atoms,
Molecules,
and Ions
Structure of the Atom: The Neutron
A number of my colleagues and I postulated that another
type of subatomic particle exists in the atomic nucleus.
Lord Ernest Rutherford
My coworkers and I carried out the bombardment of
Be (beryllium) metal with  particles. We observed that
the Be gave off high-energy radiation that we found was
unaffected by electric fields or magnets.
Sir James Chadwick
(1891-1974)
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
Atoms,
Molecules,
and Ions
Structure of the Atom: The Neutron
I gave the name neutrons to the subatomic particles that
comprised the high-energy radiation given off by the Be
metal.
A neutron is an electrically neutral particle with a mass
of 1.67493 x 10-24 g -- just slightly larger than the mass of the
positive proton (1.67262 x 10-24 g).
e-
H
relative mass = 1
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p
proton
(p)
e-
neutron
(n)
p
e-
n
He
relative
Atoms,
Molecules,
and=Ions
mass
4
Subatomic Particles
• Protons (+1) and electrons (–1) have a charge;
neutrons are neutral.
• Protons and neutrons have essentially the same
mass (relative mass 1). The mass of an electron
is so small we ignore it (relative mass 0).
• Protons and neutrons are found in the nucleus;
electrons travel around the nucleus.
Atoms,
Molecules,
and Ions
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Atomic Mass
• Atoms have extremely small masses.
• The heaviest known atoms have a
mass of approximately 4 × 10–22 g.
• A mass scale on the atomic level is
used, where an atomic mass unit
(amu) is the base unit.
1 amu = 1.66054 × 10–24 g
Atoms,
Molecules,
and Ions
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Atomic Weight Measurement
• Atomic and molecular weight can be measured
with great accuracy using a mass
spectrometer.
• Masses of atoms are compared to the carbon
atom with 6 protons and 6 neutrons (C-12).
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Symbols of Elements
 Elements are represented by a one or two letter symbol.
This is the symbol for carbon.
 All atoms of the same element have the same number of
protons, which is called the atomic number, Z. It is written
as a subscript BEFORE the symbol.
 The mass number is the total number of protons and
neutrons in the nucleus of an atom. It is written as a
superscript BEFORE the symbol.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Isotopes
• Isotopes are atoms of the same element with
different masses.
• Isotopes have different numbers of neutrons,
but the same number of protons.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
ATOMIC
NUMBER (Z)
8
O
16
The number of
protons
in the nucleus of an atom
of each element
In a neutral atom:
# of protons = # of electrons
The element considered above is oxygen. How many protons
does a neutral oxygen atom contain? How many electrons?Atoms,
Molecules,
Where are the protons located in the oxygen atom?
and Ions
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ATOMIC MASS
8
O
16
Where are neutrons located?
What is their charge?
Mass Number
(A)
The total number of
protons + neutrons
in the nucleus of an atom
of each element
In a neutral atom:
mass number =
# of protons + # of neutrons
A = Z + # neutrons
Atoms,
Molecules,
and Ions
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Atoms that have the
same atomic number
but
different
mass
numbers
Isotopes
mass number =
A
X
atomic number
=Z
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The accepted format for writing
an isotope
Z
1
3 Isotopes
of
Hydrogen
element
symbol
A
2
H
1
3
H
1
H
1
hydrogen
deuterium
tritium
1 proton
0 neutrons
1 proton
1 neutron
1 proton
2 neutrons
Atoms,
Molecules,
and Ions
Atomic number (Z) = number of protons in nucleus
Mass number (A) = number of protons + number of neutrons
= atomic number (Z) + number of neutrons
Isotopes are atoms of the same element (X) with different
numbers of neutrons in the nucleus
Mass Number
A
ZX
Atomic Number
Or it can be written as
1
1H
235
92
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2
1H
U
Element Symbol
X—A
(D)
238
92
ex) Sr-90
3
1H
U
(T)
Atoms,
Molecules,
and Ions
Try these isotopes! Determine: (a) no. of protons; (b) no. of neutrons;
(c) no. of electrons.
235
238
U
92
58
U
92
231
Fe
Th
26
90
65
130
Cu
29
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I
53
Atoms,
Molecules,
and Ions
Do You Understand Isotopes?
How many protons, neutrons, and electrons are in 146
C?
How many protons, neutrons, and electrons are in 116
C?
Atoms,
Molecules,
and Ions
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Hwk: page 73-79:
12, 17, 21, 23, 26, 27, 28, 31, 92
Atoms,
Molecules,
and Ions
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LESSON 2
Atoms,
Molecules,
and Ions
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Atomic Weight
• Because in the real world we use large amounts
of atoms and molecules, we use average masses
in calculations.
• An average mass is found using all isotopes of an
element weighted by their relative abundances.
This is the element’s atomic weight.
• That is, Atomic Weight = Ʃ [(isotope mass)
× (fractional natural abundance)]. Note:
the sum is for ALL isotopes of an element.
Atoms,
Molecules,
and Ions
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An average carbon atom consists chiefly of 2 isotopes:
12 C
6
98.9% abundant; 12.00 amu
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13
6C
1.1% abundant;
13.00335 amu
Atoms,
Molecules,
and Ions
98.9% abundant; 12.00 amu
12 C
6
13
6C
1.1% abundant;
13.00335 amu
Avg. atomic mass of C = (0.9890)(12.00 amu) + (0.0110)(13.00335 amu)
Atoms,
12.011 amu
Molecules,
and Ions
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Avg. Atomic Mass =
% isotope 1
(
)(mass in amu)
100
+···
Atoms,
Molecules,
and Ions
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Natural lithium is:
7.42% 6Li (6.015 amu)
92.58% 7Li (7.016 amu)
Average atomic mass of lithium:
7.42 x 6.015 + 92.58 x 7.016
= 6.941 amu
100
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Atomic masses of elements are indeed average masses:
1 H atom = 1.008 amu
1 O atom = 15.9994 amu
1 Fe atom = 55.85 amu
…based on elements’ isotopes and their abundances
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Atoms,
Molecules,
and Ions
Periodic Table
• The periodic
table is a
systematic
organization of the
elements.
• Elements are
arranged in order
of atomic number.
• Unlike the way we write isotopes, the atomic
number is at the TOP of a box in the periodic table.
• The atomic weight of an element appears at the
BOTTOM of the box. (They are not shown on this
Atoms,
version of the Periodic Table.)
Molecules,
and Ions
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Periodic Table
• The rows on the
periodic table are
called periods.
• Columns are
called groups.
• Elements in the
same group have
similar chemical
properties.
Atoms,
Molecules,
and Ions
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Periodicity
When one looks at the chemical properties of
elements, one notices a repeating pattern of
reactivities.
Atoms,
Molecules,
and Ions
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If F is a reactive nonmetal, which other element or
elements shown here do you expect to also be a
reactive nonmetal?
a. He and Ar
b. Be and Ca
c. H and Cl
d. Ne and Ar
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If F is a reactive nonmetal, which other element or
elements shown here do you expect to also be a
reactive nonmetal?
a. He and Ar
b. Be and Ca
c. H and Cl
d. Ne and Ar
© 2015 Pearson Education, Inc.
Intro. to the Periodic Table Movie
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Atoms,
Molecules,
and Ions
PERIODIC TABLE of the ELEMENTS
Developed in 1869 by
Dmitri Mendeleev,
a Russian chemist….
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Based on repeating
Elements 104 through
Atoms,
trends in
109 have been named
Molecules,
chemical & physical
Ions
(Rf, Db, Sg, Bh, Hs,and
Mt).
properties of elements...
Elements 104 through 109 now have names...
Bohrium
Dubnium
(named for Niels
Bohr)
(named for the
Dubna nuclear
research facility in
Russia
104
Rf
Meitnerium
105
Db
106
Sg
107
Bh
108
Hs
261.11 262.114 263.118 262.12 (265)
(named for Lise
Meitner)
109
Mt
(266)
Rutherfordium
(named for Lord
Rutherford)
Hassium
Seaborgium
(named for Glenn
T. Seaborg)
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(named for
Hassen state in
Atoms,
Germany) Molecules,
and Ions
GROUPS:
1. Vertical arrangements of elements
(a.k.a. FAMILIES)
OF ELEMENTS
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2. Possess similar chemical & physical
Atoms,
Molecules,
properties
and Ions
GROUP 1 ELEMENTS
(IA)
Lithium
(LITH-eeum)
Potassium
(po-TASS-eeum)
Cesium
(SEE-zee-um)
Francium
(FRAN-seeum)
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Hydroge
n
(HI-drojen)
Sodium
(SO-deeum)
Rubidium
(roo-BID-eeum)
ALKALI
Atoms,
(AL-kuh-lie)Molecules,
metals and Ions
GROUP 2 ELEMENTS
(IIA)
Magnesium
(mag-NEE-zeeum)
Barium
(BEAR-eeum)
Radium
(RAY-dee-um)
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Beryllium
(bur-RILL-eeum)
Calcium
(CAL-seeum)
Strontium
(STRON-teeum)
ALKALINE
EARTH
Atoms,
(AL-kuh-lin URTH)
Molecules,
metals and Ions
GROUP 16 ELEMENTS
(VIA)
Oxygen
(OX-eejen)
Sulfur
(SULL-fur)
Selenium
(sel-LEAN-eeum)
Polonium
(po-LOW-neeum)
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Tellurium
(tell-LURE-eeum)
CHALCOGENS
Atoms,
Molecules,
(CHALL-ko-jens)
and Ions
GROUP 17 ELEMENTS
(VIIA)
Fluorine
(FLOOReen)
Chlorine
(KLOR-een)
Bromine
(BRO-meen)
Iodine
(EYE-oh-deen)
Astatine
(ASS-tuh-teen)
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HALOGENS
Atoms,
Molecules,
(HAL-low-jens)
and Ions
GROUP 18 ELEMENTS
(VIIIA)
Helium
(HEE-leeum)
Neon
(NEE-on)
Argon
(ARE-gone)
Xenon
(ZEE-non)
Radon
(RAY-dawn)
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Krypton
(KRIP-tawn)
NOBLE
(or INERT)Atoms,
Molecules,
GASES and Ions
PERIODS:
1. Horizontal arrangements of elements
(or ROWS)
OF ELEMENTS
© 2015 Pearson Education, Inc.
2. Possess common characteristics
Atoms,
Molecules,
and Ions
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Main Group Elements
Representative Elements
groups 1, 2, 13  18
Atoms,
Molecules,
and Ions
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Transition elements = groups 3  12
Atoms,
Molecules,
and Ions
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The Lanthanide and Actinide series are also known as the
Rare Earth Elements or Inner transition Elements
Atoms,
Molecules,
and Ions
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In chemistry,
all elements,
natural & man-made,
are grouped into
one of three
broad classifications:
Metals:
Good conductors of heat and electricity; malleable; ductile; lustrous
Nonmetals:
Poor conductors of heat and electricity; hard
Metalloids or Semi-Metals:
Properties intermediate between those of
metals and nonmetals
Atoms,
Molecules,
and Ions
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Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Periodic Table
• Metals are on
the left side of
the periodic
table.
• Some properties
of metals
include
 shiny luster.
 conducting heat
and electricity.
 solidity (except
Atoms,
mercury). Molecules,
and Ions
© 2015 Pearson Education, Inc.
Periodic Table
• Nonmetals are
on the right side
of the periodic
table (with the
exception of H).
• They can be
solid (like
carbon), liquid
(like bromine),
or gas (like
neon) at room
temperature.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Periodic Table
• Elements on the
steplike line are
metalloids
(except Al, Po,
and At).
• Their properties
are sometimes
like metals and
sometimes like
nonmetals.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Hwk: page 73-79:
35, 41, 43, 95, 96, 100
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
LESSON 3
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Chemical Formulas
Those who do chemistry for a living use
CHEMICAL FORMULAS
to express composition of molecules and salts (i.e., ionic compounds)
in terms of chemical symbols that represent the elements.
Composition:
Which elements are
present--hydrogen
(H) & oxygen (O)
H2O
(water)
Composition:
Combining ratios of
the elements involved
-2 hydrogens : 1
oxygen
2H:1O
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Chemical Formulas
• The subscript to the right of
the symbol of an element tells
the number of atoms of that
element in one molecule of
the compound.
• Molecular compounds are
composed of molecules and
almost always contain only
nonmetals.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Diatomic Molecules
• These seven elements occur naturally
as molecules containing two atoms:
– Hydrogen
– Nitrogen
– Oxygen
– Fluorine
– Chlorine
– Bromine
– Iodine
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Types of Formulas
• Empirical formulas give the lowest wholenumber ratio of atoms of each element in a
compound.
• Molecular formulas give the exact number
of atoms of each element in a compound.
• If we know the molecular formula of a
compound, we can determine its empirical
formula. The converse is not true!
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
CHEMICAL FORMULAS
2
types
MOLECULAR
EMPIRICAL
C6H12O6 glucose
CH2O
Exact no. of atoms
of each element
in smallest unit
of substance
© 2015 Pearson Education, Inc.
Elements present
in simplest
whole-number Atoms,
ratio
Molecules,
of their atoms
and Ions
A molecular formula shows the exact number of
atoms of each element in the smallest unit of a
substance
An empirical formula shows the simplest
whole-number ratio of the atoms in a substance
molecular
empirical
H2O
H2O
C6H12O6
CH2O
O3
O
N2H4
NH2
© 2015 Pearson Education, Inc.
Atoms,
Molecules,
and Ions
2.6
The simplest chemical formulas
EMPIRICAL
formulas
Tell us which elements are present and
simplest whole-number ratio of their atoms
NOT NECESSARILY the actual number
of atoms in a given molecule
Subscript “1” is understood & not written
when there’s only ONE atom of an element
present.
C2H4O2
CH2O
empirical
formula
© 2015 Pearson Education, Inc.
C3H6O3
C6H12O6
molecular
formulas
Atoms,
Molecules,
and Ions
MOLECULAR
formulas
Exact number of atoms of each element
in the smallest unit of a substance
H2
hydrogen
O2
oxygen
Allotropes
O3
ozone
H2O
water
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2 or more
distinct
forms of
an
element
Atoms,
Molecules,
and Ions
Allotropes
Carbon
Diamond
Graphite
Fullerenes
Atoms,
Molecules,
and Ions
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H2O
water
NH3
ammonia
CO2
carbon dioxide
CH4
methane
© 2015 Pearson Education, Inc.
For these molecules,
and many more, the
empirical AND
molecular formulas
are the same.
Atoms,
Molecules,
and Ions
Types of Formulas
• Structural formulas show
the order in which atoms are
attached. They do NOT
depict the three-dimensional
shape of molecules.
• Perspective drawings also
show the three-dimensional
order of the atoms in a
compound. These are also
demonstrated using models.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Chemical Formulas and Molecular Models
OR
“How Do We Visualize Something as Ridiculously Small as a Molecule?”
H
CH4
H C
Molecular
formula
H
Structural
formula
H
H
USE
MOLECULAR
MODELS!!!
H
C
H
© 2015 Pearson Education, Inc.
H
Ball-and-stick
model
Space-filling
Atoms,
model
Molecules,
and Ions
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
2.6
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Which model, the ball-and-stick or the spacefilling, more effectively shows the angles between
bonds around a central atom?
a. Ball-and-stick
b. Space-filling
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Which model, the ball-and-stick or the spacefilling, more effectively shows the angles between
bonds around a central atom?
a. Ball-and-stick
b. Space-filling
© 2015 Pearson Education, Inc.
Ions
• When an atom of a group of atoms loses or gains
electrons, it becomes an ion.
• Cations are formed when at least one electron is lost.
Monatomic cations are formed by metals.
• Anions are formed when at least one electron is gained.
Atoms,
Monatomic anions are formed by nonmetals.
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Ions
• An atom or group of atoms having a net positive or negative
charge.
Two types of ions...
CATIONS
ANIONS
Ions with a net positive
charge.
Formed by LOSS of one or
more electrons from a
neutral atom.
Ions with a net negative
charge.
Formed by GAIN of one or
more electrons by a
neutral atom.
Monatomic ions: have only 1 atom
Polyatomic ions: more than 1 atom
© 2015 Pearson Education, Inc.
Atoms,
Molecules,
and Ions
A monatomic ion contains only one atom
Na+, Cl-, Ca2+, O2-, Al3+, N3-
A polyatomic ion contains more than one atom
OH-, CN-, NH4+, NO3-
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
2.5
Ions
-1e-
Na+
Na
CATION
Sodium ion
+1e-
Cl
Cl-
ANION
Chloride ion
IONIC
COMPOUND
Na+
+
Cl-
Na+
Cl-
Formed from
cations and
Atoms,
anionsMolecules,
and Ions
© 2015 Pearson Education, Inc.
Sodium chloride
(1) The most common ions for silver, zinc, and
scandium are Ag+, Zn2+, and Sc3+. Locate the boxes
in which you would place these ions in this table.
(1)
Ag+
Zn2+
Sc3+
a. 2B
3B
4B
b. 1B
2B
3B
c. 1B
3B
2B
d. 4B
3B
2B
© 2015 Pearson Education, Inc.
(1) The most common ions for silver, zinc, and
scandium are Ag+, Zn2+, and Sc3+. Locate the boxes
in which you would place these ions in this table.
(1)
Ag+
Zn2+
Sc3+
a. 2B
3B
4B
b. 1B
2B
3B
c. 1B
3B
2B
d. 4B
3B
2B
© 2015 Pearson Education, Inc.
(2) Which of these ions have the same number of
electrons as a noble gas element?
(2)
a. Ag+
b. Zn2+
c. Sc3+
d. (B) and (C)
© 2015 Pearson Education, Inc.
(2) Which of these ions have the same number of
electrons as a noble gas element?
(2)
a. Ag+
b. Zn2+
c. Sc3+
d. (B) and (C)
© 2015 Pearson Education, Inc.
Common Cations
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Common Anions
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Examples of Ions **
Monatomic Cations
Li+
Na+
Mg2+
Ba2+
Cr3+
Cr6+
Fe2+
Fe3+
Al3+
Pb2+
Pb4+
lithium ion
sodium ion
magnesium ion
barium ion
chromium (III) ion*
chromium (VI) ion*
iron (II) ion*
iron (III) ion*
aluminum ion
lead (II) ion*
lead (IV) ion*
Monatomic Anions
FClBrIO2S2N3P3C4-
fluoride ion
chloride ion
bromide ion
iodide ion
oxide ion
sulfide ion
nitride ion
phosphide ion
carbide ion
Polyatomic Ions
NH4+
PO43SO42CO32NO3C2H3O2OHCN-
ammonium ion
phosphate ion
sulfate ion
carbonate ion
nitrate ion
acetate ion
hydroxide ion
cyanide ion
* For cations with more than
one charge possible, a Roman
numeral is used to denote the
charge on the cation.
Atoms,
Molecules,
and Ions
© 2015 Pearson
Inc. 2.11, p. 49, Chang 7th ed.)
** Refer
alsoEducation,
to Figure
MONOATOMIC IONS
Hydride
HHydrogen
H+
CATIONS
Lithium
Li+
Beryllium
Be2+
Sodium
Na+
Magnesium
Mg2+
Potassium
K+
ANIONS
Nitride
N3-
Oxide
O2-
Fluoride
F-
Phosphide
P3-
Sulfide
S2-
Chloride
Cl-
Calcium
Ca2+
Selenide
Se2-
Bromide
Br-
Rubidium
Rb+
Strontium
Sr2+
Telluride
Te2-
Iodide
I-
Cesium
Cs+
Barium
Ba2+
© 2015 Pearson Education, Inc.
Carbide
C4-
Aluminum
Al3+
Hydrogen can be
both a cation and
an anion.
Atoms,
Molecules,
and Ions
METALS THAT FORM MORE
THAN ONE CATION*
Metal IonStock Name Metal IonStock Name
Cr2+
chromium (II)
Mn2+
manganese (II)
Cr3+
chromium (III)
Mn3+
manganese (III)
Cr6+
chromium (VI)
Mn4+
manganese (IV)
V3+
vanadium (III)
Mn6+
manganese (VI)
V5+
vanadium (V)
Mn7+
manganese (VII)
Fe2+
iron (II)
Cu+
copper (I)
Fe3+
iron (III)
Cu2+
copper (II)
Pb2+
lead (II)
Sn2+
tin (II)
Pb4+
lead (IV)
Sn4+
tin (IV)
Au+
gold (I)
Co2+
cobalt (II)
gold (III)
Co3+
Au3+
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cobalt (III)
Atoms,
Molecules,
and Ions
Polyatomic Ions--A Partial List
NH4+ ammonium
NO3- nitrate
NO2- nitrite
SO42- sulfate
SO32- sulfite
HSO4- bisulfate
PO43- phosphate
PO33- phosphite
HPO42- hydrogen phosphate
H2PO42- dihydrogen phosphate
OH- hydroxide
CN- cyanide
C2H3O2- acetate
CO32- carbonate
HCO3- bicarbonate
ClO4ClO3ClO2ClO-
perchlorate
chlorate
chlorite
hypochlorite
MnO4- permanganate
Cr2O72- dichromate
CrO42- chromate
O22peroxide
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Ionic Compounds
Ionic compounds (such as NaCl) are generally
formed between metals and nonmetals.
Electrons are transferred from the metal to the
nonmetal. The oppositely charged ions attract
each other. Only empirical formulas are written.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Writing Formulas
• Because compounds are electrically neutral,
one can determine the formula of a
compound this way:
– The charge on the cation becomes the subscript
on the anion.
– The charge on the anion becomes the subscript
on the cation.
– If these subscripts are not in the lowest wholenumber ratio, divide them by the greatest common
Atoms,
factor.
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Formulas of Ionic Compounds
• Usually the same as their empirical formulas
• Made up of ions -- actually, a 1:1 ratio of cations to anions
• Ionic compound itself is electrically neutral -SUM OF POSITIVE and NEGATIVE
CHARGES MUST EQUAL ZERO!!
• PRINCIPLE OF CHARGE BALANCE applied to formulas of
ionic compounds:
The subscript of the cation is numerically equal to the charge on
the anion, AND the subscript of the anion is numerically equal to
the charge on the cation.
MORE TO COME…
© 2015 Pearson Education, Inc.
Atoms,
Molecules,
and Ions
CHARGE BALANCE: How it works
1. Ionic compounds are
electrically NEUTRAL; that
is, their overall charge equals
ZERO.
2. Simple anions have known
negative charges.
3. The SUM of the positive
charge from the cation and
the negative charge of the
anion must equal ZERO.
This is the principle of charge
balance.
Examples: CrO3 and CrCl3
• Both CrO3 and CrCl3 have an overall charge
of zero.
• The oxide anion, O2-, in CrO3 has a -2 charge.
The chloride anion, Cl-, in CrCl3 has a -1
charge.
Use algebra to set up an expression to solve for
the charge on Cr for each compound:
• Let x = charge on Cr in CrCl3.
• (1)x + (3)(-1) = 0
OR x + (3)(-1) = 0
o. of metal cations)(charge on cation) + (no. of nonmetal anions)(charge
© 2015 Pearson Education, Inc.
Atoms,
Molecules,
on and
anion)
Ions
=
CHARGE BALANCE: How it works
4. Determine the charge on
the metal cation.
x + (3)(-1) = 0
x - 3 = 0 ; x = 3  This is the charge on
Cr in CrCl3.
Now, you try this one:
What is the charge on Cr in CrO3?
o. of metal cations)(charge on cation) + (no. of nonmetal anions)(charge
© 2015 Pearson Education, Inc.
Atoms,
Molecules,
on and
anion)
Ions
=
Formula of Ionic Compounds
2 x +3 = +6
3 x -2 = -6
Al2O3
Al3+
1 x +2 = +2
Ca2+
1 x +2 = +2
Na+
© 2015 Pearson Education, Inc.
O22 x -1 = -2
CaBr2
Br1 x -2 = -2
Na2CO3
CO32-
Atoms,
Molecules,
and Ions
Formulas of Ionic Compounds
• OK, so we know the charges on the cation and anion, respectively…
So, how do we write formulas of ionic compounds in this case?
o. of metal cations)(charge on cation) + (no. of nonmetal anions)(charge on anion) =
Try these…
potassium
iodide
© 2015
Pearson Education, Inc.
zinc
fluoride
Atoms,
ironMolecules,
(III)
and Ions
oxide
(d) Magnesium sulfide
(e) cobalt(II) chloride
(f) Aluminum oxide
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
(d) Strontium hydroxide
(e) Sodium carbonate
(f) Ammonium phosphate
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
What is the formula for mercury (I) carbide?
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Homework is a worksheet
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Hwk: page 73-79:
5, 7, 47, 49, 51, 53, 55, 57, 59, 61, 63, 65
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
LESSON 4
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Inorganic Nomenclature
• Write the name of the cation. If the cation
can have more than one possible charge,
write the charge as a Roman numeral in
parentheses.
• If the anion is an element, change its
ending to -ide; if the anion is a polyatomic
ion, simply write the name of the
polyatomic ion.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Patterns in Oxyanion Nomenclature
• When there are two oxyanions involving the
same element
– the one with fewer oxygens ends in -ite.
– the one with more oxygens ends in -ate.
• NO2− : nitrite; NO3− : nitrate
• SO32− : sulfite; SO42− : sulfate
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Patterns in Oxyanion Nomenclature
• Central atoms on the second row have a
bond to, at most, three oxygens; those on the
third row take up to four.
• Charges increase as you go from right to left.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Patterns in Oxyanion Nomenclature
• The one with the second fewest oxygens ends in -ite: ClO2− is
chlorite.
• The one with the second most oxygens ends in -ate: ClO3− is
chlorate.
• The one with the fewest oxygens has the prefix hypo- and
ends in -ite: ClO− is hypochlorite.
• The one with the most oxygens has the prefix per- and ends
in -ate: ClO4− is perchlorate.
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Name the anion obtained by removing one oxygen
atom from the perbromate ion, BrO4–.
a. Hypobromite ion
b. Bromite ion
c. Bromate ion
d. Bromine ion
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Name the anion obtained by removing one oxygen
atom from the perbromate ion, BrO4–.
a. Hypobromite ion
b. Bromite ion
c. Bromate ion
d. Bromine ion
© 2015 Pearson Education, Inc.
Acid Nomenclature
• If the anion in the acid ends
in -ide, change the ending
to -ic acid and add the
prefix hydro-.
– HCl: hydrochloric acid
– HBr: hydrobromic acid
– HI: hydroiodic acid
• If the anion ends in -ite, change the ending to -ous acid.
– HClO: hypochlorous acid
– HClO2: chlorous acid
• If the anion ends in -ate, change the ending to -ic acid.
– HClO3: chloric acid
Atoms,
– HClO4: perchloric acid
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Nomenclature of
Binary Molecular Compounds
• The name of the element
farther to the left in the
periodic table (closer to
the metals) or lower in the
same group is usually
written first.
• A prefix is used to denote
the number of atoms of
each element in the
compound (mono- is not
used on the first element
Atoms,
listed, however).
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Nomenclature of Binary Compounds
• The ending on the second element is changed
to -ide.
– CO2: carbon dioxide
– CCl4: carbon tetrachloride
• If the prefix ends with a or o and the name of
the element begins with a vowel, the two
successive vowels are often elided into one.
– N2O5: dinitrogen pentoxide
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Nomenclature of Organic Compounds
• Organic chemistry is the study of carbon.
• Organic chemistry has its own system of nomenclature.
• The simplest hydrocarbons (compounds containing only
carbon and hydrogen) are alkanes.
• The first part of the names just listed correspond to the
number of carbons (meth- = 1, eth- = 2, prop- = 3, etc.).
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Nomenclature of Organic Compounds
• When a hydrogen in an alkane is replaced with
something else (a functional group, like -OH in
the compounds above), the name is derived from
the name of the alkane.
• The ending denotes the type of compound.
– An alcohol ends in -ol.
© 2015 Pearson Education, Inc.
Atoms,
Molecules,
and Ions
• Hwk: page 73-79:
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
Review Questions
Chapter 2
Atoms,
Molecules,
and Ions
© 2015 Pearson Education, Inc.
The nucleus of an atom
contains
a.
b.
c.
d.
protons and neutrons.
protons and electrons.
electrons and neutrons.
protons, neutrons, and electrons.
© 2015 Pearson Education, Inc.
The nucleus of an atom
contains
a.
b.
c.
d.
protons and neutrons.
protons and electrons.
electrons and neutrons.
protons, neutrons, and electrons.
© 2015 Pearson Education, Inc.
Two atoms with the same
atomic number but different
mass numbers are called
a.
b.
c.
d.
mutants.
isomers.
isotopes.
symbiots.
© 2015 Pearson Education, Inc.
Two atoms with the same
atomic number but different
mass numbers are called
a.
b.
c.
d.
mutants.
isomers.
isotopes.
symbiots.
© 2015 Pearson Education, Inc.
Select the incorrect statement
about the mass and volume of
an atom.
a. The mass is determined mostly by the
protons and neutrons.
b. The volume is mostly empty space.
c. The mass is concentrated in the nucleus.
d. The volume is determined by the
arrangement of the protons.
© 2015 Pearson Education, Inc.
Select the incorrect statement
about the mass and volume of
an atom.
a. The mass is determined mostly by the
protons and neutrons.
b. The volume is mostly empty space.
c. The mass is concentrated in the nucleus.
d. The volume is determined by the
arrangement of the protons.
© 2015 Pearson Education, Inc.
For an atom of fluorine, the
atomic number is ___ and the
average atomic mass is ___.
a.
b.
c.
d.
9; 18.988 amu
18.998; 9 amu
10; 19 g
9; 9 g
© 2015 Pearson Education, Inc.
For an atom of fluorine, the
atomic number is ___ and the
average atomic mass is ___.
a.
b.
c.
d.
9; 18.988 amu
18.998; 9 amu
10; 19 g
9; 9 g
© 2015 Pearson Education, Inc.
Atomic weights on the periodic
table are decimal numbers
instead of integers because
a. the number of protons + neutrons
determines atomic weight.
b. of the existence of isotopes.
c. of the very small mass of electrons
compared to protons and neutrons.
d. the number of protons + electrons
determines atomic weight.
© 2015 Pearson Education, Inc.
Atomic weights on the periodic
table are decimal numbers
instead of integers because
a. the number of protons + neutrons
determines atomic weight.
b. of the existence of isotopes.
c. of the very small mass of electrons
compared to protons and neutrons.
d. the number of protons + electrons
determines atomic weight.
© 2015 Pearson Education, Inc.
The elements found on the
right side of the periodic table
tend to ______ electrons.
a.
b.
c.
d.
gain
lose
keep
share
© 2015 Pearson Education, Inc.
The elements found on the
right side of the periodic table
tend to ______ electrons.
a.
b.
c.
d.
gain
lose
keep
share
© 2015 Pearson Education, Inc.
Metals and nonmetals react to
form ________ compounds.
a.
b.
c.
d.
molecular
mixed
empirical
ionic
© 2015 Pearson Education, Inc.
Metals and nonmetals react to
form ________ compounds.
a.
b.
c.
d.
molecular
mixed
empirical
ionic
© 2015 Pearson Education, Inc.
Positive ions are called
a.
b.
c.
d.
positrons.
anions.
cations.
nucleons.
© 2015 Pearson Education, Inc.
Positive ions are called
a.
b.
c.
d.
positrons.
anions.
cations.
nucleons.
© 2015 Pearson Education, Inc.
Compounds composed only of
carbon and hydrogen are
called
a.
b.
c.
d.
binary acids.
carbohydrates.
hydrocarbons.
alkanes.
© 2015 Pearson Education, Inc.
Compounds composed only of
carbon and hydrogen are
called
a.
b.
c.
d.
binary acids.
carbohydrates.
hydrocarbons.
alkanes.
© 2015 Pearson Education, Inc.
The elements located in Group
VIIA (Group 17) on the periodic
table are called
a.
b.
c.
d.
alkali metals.
noble gases.
chalcogens.
halogens.
© 2015 Pearson Education, Inc.
The elements located in Group
VIIA (Group 17) on the periodic
table are called
a.
b.
c.
d.
alkali metals.
noble gases.
chalcogens.
halogens.
© 2015 Pearson Education, Inc.
Which of the formulas below
does not represent a compound
that actually exists?
a.
b.
c.
d.
CaCO3
H 2O 2
KMnO4
Na2PO3
© 2015 Pearson Education, Inc.
Which of the formulas below
does not represent a compound
that actually exists?
a.
b.
c.
d.
CaCO3
H 2O 2
KMnO4
Na2PO3
© 2015 Pearson Education, Inc.
Which name is incorrectly
paired with the formula?
a.
b.
c.
d.
hydroxide ion; OH–
barium(II) chloride; BaCl2
ammonia; NH3
sulfur dioxide; SO2
© 2015 Pearson Education, Inc.
Which name is incorrectly
paired with the formula?
a.
b.
c.
d.
hydroxide ion; OH–
barium(II) chloride; BaCl2
ammonia; NH3
sulfur dioxide; SO2
© 2015 Pearson Education, Inc.
Acids produce _____ ions.
a.
b.
c.
d.
OH–1
OH+1
H+1
H–1
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Acids produce _____ ions.
a.
b.
c.
d.
OH–1
OH+1
H+1
H–1
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NaOCl is named
a.
b.
c.
d.
sodium chlorate.
sodium chlorite.
sodium perchlorate.
sodium hypochlorite.
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NaOCl is named
a.
b.
c.
d.
sodium chlorate.
sodium chlorite.
sodium perchlorate.
sodium hypochlorite.
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LiNO3 is named
a.
b.
c.
d.
lithium nitrate.
lanthanum nitrate.
lanthanum nitrite.
lithium nitrite.
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LiNO3 is named
a.
b.
c.
d.
lithium nitrate.
lanthanum nitrate.
lanthanum nitrite.
lithium nitrite.
© 2015 Pearson Education, Inc.
The formula for aluminum
carbonate is
a.
b.
c.
d.
Al2(CO3)3.
AlCO3.
Al2C3.
Al3(CO3)2.
© 2015 Pearson Education, Inc.
The formula for aluminum
carbonate is
a.
b.
c.
d.
Al2(CO3)3.
AlCO3.
Al2C3.
Al3(CO3)2.
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Fe2O3 is named
a.
b.
c.
d.
diiron trioxide.
iron(III) oxide.
ferrous oxide.
ironic oxide.
© 2015 Pearson Education, Inc.
Fe2O3 is named
a.
b.
c.
d.
diiron trioxide.
iron(III) oxide.
ferrous oxide.
ironic oxide.
© 2015 Pearson Education, Inc.
Which acid is not an oxyacid?
a.
b.
c.
d.
hydrochloric acid
nitric acid
sulfurous acid
acetic acid
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Which acid is not an oxyacid?
a.
b.
c.
d.
hydrochloric acid
nitric acid
sulfurous acid
acetic acid
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HIO4 is named
a.
b.
c.
d.
iodic acid.
iodous acid.
periodic acid.
hydrogen iodate.
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HIO4 is named
a.
b.
c.
d.
iodic acid.
iodous acid.
periodic acid.
hydrogen iodate.
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Cl2O7 is named
a.
b.
c.
d.
chlorine(VII) oxide.
dichlorine hexaoxide.
dichlorine heptaoxide.
bichlorine heptaoxide.
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Cl2O7 is named
a.
b.
c.
d.
chlorine(VII) oxide.
dichlorine hexaoxide.
dichlorine heptaoxide.
bichlorine heptaoxide.
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C3H8 is named
a.
b.
c.
d.
ethane.
propane.
propanol.
pentane.
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C3H8 is named
a.
b.
c.
d.
ethane.
propane.
propanol.
pentane.
© 2015 Pearson Education, Inc.
TEST
© 2015 Pearson Education, Inc.