Chemistry
• Demetri Mendelev and the Periodic Table
Periods and Groups
• The Periodic Table arranges elements in rows,
called periods, and columns, called groups.
The order of the elements is determined by
atomic number.
Meet the Elements
• Meet the Elements Video
Types of
Matter
Atom
Types of
Matter
Atom
Element
Compound
Element
Compound
Molecule
Mixture
Molecule
Mixture
Types of
Matter
Atom
Types of
Matter
Atom
Element
Compound
Element
Compound
Molecule
Mixture
Molecule
Mixture
Types of Matter
Chemistry Unit 1
Structure of
an Atom
Protons and
an Atoms
identity
Valence
Electrons and
Reactivity
The Periodic
Table
Chemistry Unit 2
Chemical
Formulas
Chemical
Reactions
Chemical
Equations
Law of
Conservation
of Mass
Chemistry Vocabulary, Unit 1, part 1
atom: the smallest particle of an element that has all the properties
of that element
element: a pure substance, made up of similar atoms, that cannot be
broken down by chemical means
Chemistry Vocabulary, Unit 1, part 2
Periodic Table: a logical arrangement of the elements into rows
and columns; an element’s position in the Periodic Table can be
used to predict its properties
group: a column of the Periodic Table; elements in the same
group have similar properties
nucleus: the center of an atom, which contains protons and neutrons
period: a row of the Periodic Table
proton: the subatomic particle in the nucleus that has a positive
electric charge
valence electrons: the outermost electrons of an atom, which
help determine an element’s chemical properties
neutron: the subatomic particle in the nucleus that has no electric
charge
metal: an element that is typically dense, shiny, strong, and a
good conductor of heat and electricity
electron cloud: the region around the nucleus where electrons are
found
electron: the negatively charged subatomic particle that exists in a
cloud surrounding the nucleus
unified atomic mass unit (u): the unit for measuring the mass of
atoms
electric charge: a property of matter that causes it to experience a
force near other charged matter
valence electrons: the outermost electrons of an atom, which help
determine an element’s chemical properties
ion: an atom or molecule that has gained or lost one or more
electrons
chemical bond: an attractive force between atoms or ions, formed by
the sharing or transfer of valence electrons
nonmetal: an element that typically is not dense, and is dull,
brittle, and a poor conductor of heat and electricity
metalloid: an element that has properties between those of a
metal and nonmetal; also called a semimetal
pure substance: matter that has the same chemical composition
throughout
compound: a substance that forms when two or more elements
join chemically
molecule: a group of two or more atoms held together by
chemical bonds
chemical formula: a group of chemical symbols and numbers
that shows the kinds and numbers of atoms in a molecule
Protons,
Neutrons and
Electrons
The Hierarchical
Relationship of
Atomic Structure
Atoms
Molecules
Minerals
Mineral
Rocks
Neutrons
Electrons
Protons
Earth
Element
• A pure substance, made
up of similar atoms, that
cannot be broken down
by chemical means
• An element’s identity is
determined by the
number of protons.
• Interactive Periodic Table
http://www.ptable.com/
What do you know about
chemistry?
Atom
Nucleus
• Nucleus is a term used
to describe the control
center in an animal
cell (Biology)
• Nucleus is the term to
describe the very
dense region at the
center of an atom
(Chemistry)
Is this
an
animal
or a
plant
cell?
Components of an Atom
• Proton
• Neutron
• Electron
• All about Atoms
Protons
• Have a positive
charge
• Mass =1u or 1amu
(unified atomic mass)
• Located in the nucleus
• The number of
protons determines
the elements identity
Captain Proton
A proton is made
up of two up
quarks and one
down quark
Neutrons
• Neutral Charge
• Mass 1u
• Located in the
Nucleus
• Elements with a
variable number of
neutrons are called
isotopes
Electrons and the Electron Cloud
•
•
•
•
Electron Mass: Close to 0 u
Negative Charge
located in the Electron Cloud
Atoms with a different number of
electrons are called ions.
• The Electrons cloud is subdivided
into shells
• The shells hold a fixed amount of
electrons
– 1st shell holds 2 electrons
– 2nd shell holds 8 electrons
– 3rd shell holds 8 electrons
How to calculate Atomic Mass and
Atomic Number.
APE MAN
• Atomic Number = #Protons = #Electrons
• Mass Number- Atomic Number = Neutrons
Atomic Components
Sub-Atomic Particle
Electrical Charge
Mass
Location in Atom
Proton
+
1u
Nucleus
Neutron
neutral
1u
Nucleus
Electron
-
0u
Electron Cloud
If the number of protons change, you have a different element.
If the number of neutrons change, you have an isotope.
If the number of electrons change, you have an ion.
Bohr Model
Bohr Model
Bohr Model
Bohr Model
Name the Atom
Draw the Atomic Structure
P
E
N
Dice Roll
1
2
3
4
5
6
Dice Roll
1
2
3
4
5
6
Dice Roll
1
2
3
4
5
6
Action
Metal, Metalloid or Non-Metal?
Draw the Atomic Structure
What period is the element in?
What group is the element in?
Draw the Lewis Dot Structure
Draw the Atomic Structure
Action
Metal, Metalloid or Non-Metal?
Draw the Atomic Structure
What period is the element in?
What group is the element in?
Draw the Lewis Dot Structure
Draw the atomi
Action
Metal, Metalloid or Non-Metal?
Draw the Atomic Structure
What period is the element in?
What group is the element in?
Draw the Lewis Dot Structure
Build the Atom
Dice Roll
1
2
3
4
5
6
Dice Roll
1
2
3
4
5
6
Dice Roll
1
2
3
4
5
6
Action
Metal, Metalloid or Non-Metal?
Draw the Atomic Structure
What period is the element in?
What group is the element in?
Draw the Lewis Dot Structure
Build the Atom
Action
Metal, Metalloid or Non-Metal?
Draw the Atomic Structure
What period is the element in?
What group is the element in?
Draw the Lewis Dot Structure
Build the Atom
Action
Metal, Metalloid or Non-Metal?
Draw the Atomic Structure
What period is the element in?
What group is the element in?
Draw the Lewis Dot Structure
Build the Atom
H
H
H
H
H
He
He
He
He
He
Li
Li
Li
Li
Li
B
B
B
B
B
Be
Be
Be
Be
Be
C
C
C
C
C
N
N
N
N
N
O
O
O
O
O
F
F
F
F
F
Ne
Ne
Ne
Ne
Ne
Na
Na
Na
Na
Na
Mg
Mg
Mg
Mg
Mg
Al
Al
Al
Al
Al
Si
Si
Si
Si
Si
P
P
P
P
P
Si
Si
Si
Si
Si
Cl
Cl
Cl
Cl
Cl
Ar
Ar
Ar
Ar
Ar
Chemistry Review Stations
Review
Station
2 sentences
Stamp
Chemistry Review Stations
Review
Station
Build an
Atom
Build an
Atom
Petri Dish
Elements
Petri Dish
Elements
Conversation
with a
Teacher
Conversation
with a
Teacher
2 sentences
Stamp
Build an Atom
Element
`
1.
2.
3.
Draw an Element
Build the Atom
Roll the dice and illustrate your paper
Action
Build an Atom
Element
1.
2.
3.
Draw an Element
Build the Atom
Roll the dice and illustrate your paper
Action
Subatomic Particle Mass of Particles
____ protons
____electrons
_____neutrons
Total Mass of
Electric Charge
Build the Atom
The formation of Salt
Valence Electrons
• Valence Electrons determine an elements
chemical properties, including reactivity.
• Valence Electrons refer to the number of
electrons in their outer shell
Lewis Dot Structure
Ne
Si
B
H
O
Be
He
C
Li
Valence Electrons
• The Lewis dot structure shows just the valence
electrons
• The valence electrons are the electrons in the
out shell
• The number valence electrons in the outer
shell determine the reactivity
Lewis Dot Structure
Noble Gases
Chemistry Vocabulary, Unit 1, Part 2
Periodic Table: a logical arrangement of the elements into rows and columns; an element’s
position in the Periodic Table can be used to predict its properties
group: a column of the Periodic Table; elements in the same group have similar properties
period: a row of the Periodic Table
valence electrons: the outermost electrons of an atom, which help determine an element’s
chemical properties
metal: an element that is typically dense, shiny, strong, and a good conductor of heat and
electricity
nonmetal: an element that typically is not dense, and is dull, brittle, and a poor conductor
of heat and electricity
metalloid: an element that has properties between those of a metal and nonmetal; also
called a semimetal
pure substance: matter that has the same chemical composition throughout
compound: a substance that forms when two or more elements join chemically
molecule: a group of two or more atoms held together by chemical bonds
chemical formula: a group of chemical symbols and numbers that shows the kinds and
numbers of atoms in a molecule
METALS, NONMETALS,
METALLOIDS, &
NOBLE GASES
FOUR SECTION FOLDABLE
ADVANCED ORGANIZER
Metals, Non-metals and Metalloids
• The Periodic Table can be used to predict
many properties of elements.
– Metals are located on the left side and in the
center of the table, while nonmetals are clustered
on the right side.
– A staircase-like line divides the two groups.
– Elements called metalloids, which have some
properties of metals and some properties of
nonmetals, are located along this line.
Metals
Metalloids
Non-Metals
Metals
Color metals non-metals and metalloids.
Cut apart the metals, non=metals and metalloids
Paste each section under its heading
Draw columns to separate the categories.
Metalloids
Non-Metals
Color metals non-metals and metalloids.
Cut apart the metals, non=metals and metalloids
Paste each section under its heading
Draw columns to separate the categories.
Examples:
Examples:
Examples:
Examples:
Examples:
Examples:
Groups:
Groups:
Groups:
Groups:
Groups:
Groups:
Properties:
Properties:
Properties:
Properties:
Properties:
Properties:
PROPERTIES OF METALS
• Most elements are metals
• Metals have few electrons in their outer energy level
• Metals are solid at room temperature except Mercury
which is a liquid
• Metals are good conductors of heat and electricity
• Metals are malleable which means they can be
flattened into thin sheets
• Metals are ductile which means they can be drawn
into thin wires
• Metals are shiny
PROPERTIES OF NONMETALS
• Nonmetals are located right of the Zig Zag line
• Nonmetals have almost a complete set of electrons in
their outer energy level
• Nonmetals are mostly gases at room temperature
• Nonmetals are not good conductors of heat &
electricity
• Nonmetals are not malleable
• Nonmetals are not ductile – they are brittle and will
break or shatter when hit with a hammer
• Nonmetals are not shiny
PROPERTIES OF METALLOIDS
• Metalloids are also called semiconductors
• Metalloids border the Stairs
• Metalloids have a ½ complete set of
electrons in their outer energy level
• Metalloids have some properties of
metals and some properties of
nonmetals.
EXAMPLES OF METALLOIDS
• Tellurium-shiny but brittle
• Silicon-semiconductor
• Boron-hard but brittle and a good
conductor of electricity
PROPERTIES OF NOBLE GASES
• Noble Gases are Family 18
• Noble Gases have a complete set of
electrons in their outer energy level – all
but Helium have 8. Helium has 2.
• Noble Gases are gases at room
temperature
• Noble Gases are nonmetals
PROPERTIES OF NOBLE GASES
•
•
•
•
Noble Gases are colorless
Noble Gases are odorless
Noble Gases are unreactive
Noble Gases are found in very small
amounts on Earth
EXAMPLES OF NOBLE GASES
•
•
•
•
•
Helium
Argon
Krypton
Xenon
Radon (Radioactive gas)
• The periods grow in size on the table from top to
bottom. The first period has only two elements,
hydrogen (atomic number 1) and helium (atomic
number 2). The second and third periods each
contain eight elements, and the next two periods
each contain 18 elements.
• The last two periods contain 32 elements. To
make the table easier to read, some of these
elements are placed at the bottom of the table.
• The table is organized so that elements with similar
configurations of valence electrons are placed in the
same column, or group.
– Atoms of elements in Group 1 (including hydrogen, lithium,
and sodium) each have one valence electron.
– Atoms of elements in Group 17 (including fluorine,
chlorine, and bromine) each have seven valence electrons.
•
• Valence electrons help determine the
chemical properties of an element. This
means that the elements in a group all have
similar chemical properties.
Metals, Metalloids and Non-Metals
Metalloids
Noble Gases
Metalloids
Noble Gases
Metals
Non-Metals
Metals
Non-Metals
Metals
Metalloids
Non-Metals
Noble Gases
Electrons
Components
of an Atom
Protons
Neutrons
Metalloids
Noble Gases
Metalloids
Noble Gases
Metals
Non-Metals
Metals
Non-Metals
Glue Nows!
Atomic
Structure
Atomic
Structure
As you answer these questions, remember that atoms tend to
be most stable when their outer energy level is full with
electrons. They gain, lose, or share their outer electrons—
called valence electrons—to achieve a full outer set.
As you answer these questions, remember that atoms tend to
be most stable when their outer energy level is full with
electrons. They gain, lose, or share their outer electrons—
called valence electrons—to achieve a full outer set.
1. Of the 10 atoms you modeled, which 2 are the most stable? Explain.
1. Of the 10 atoms you modeled, which 2 are the most stable? Explain.
2. Look at the electron structures for lithium and fluorine. In a chemical
reaction, the valence electron of a lithium atom transfers to the fluorine
atom. This changes both atoms into ions. Explain why this reaction
occurs.
2. Look at the electron structures for lithium and fluorine. In a chemical
reaction, the valence electron of a lithium atom transfers to the fluorine
atom. This changes both atoms into ions. Explain why this reaction
occurs.
3. When hydrogen and oxygen react, they combine in a 2-to-1 ratio to
form a molecule of water (H 2 O). In this reaction, each of the 2 hydrogen
atoms shares its valence electron with 1 oxygen atom. Explain why this
reaction takes place in terms of the number of valence electrons.
3. When hydrogen and oxygen react, they combine in a 2-to-1 ratio to
form a molecule of water (H 2 O). In this reaction, each of the 2 hydrogen
atoms shares its valence electron with 1 oxygen atom. Explain why this
reaction takes place in terms of the number of valence electrons.
Sub-Atomic
Particle
Electrical
Charge
Mass
Location in
Atom
Sub-Atomic
Particle
Electrical
Charge
Mass
Location in
Atom
SubAtomic
Particle
Electrical
Charge
Mass
Location in
Atom
8. a
•
•
Key Concepts
An atom is the basic component of matter. All the atoms of a specific element, such as hydrogen, are similar.
Elements are the basic substances or building blocks that make other substances. For example, the elements
hydrogen and oxygen combine to form water. The elements sodium and chlorine combine to form table salt.
•
The center of an atom is called the nucleus. The nucleus contains smaller particles called protons and neutrons.
The electron cloud contains electrons that surround the nucleus. The electrons can be found anywhere in the
cloud, but are more likely to be found in some places than in others.
The mass of the particles of an atom are recorded in unified atomic mass units (u). The mass of each proton and
neutron is very close to 1 u. Electrons have almost no mass.
•
•
Some atoms in an element can have different numbers of neutrons. Because of this, the average atomic mass of
the atoms for that element is used to describe atoms. For example, about 99 percent of carbon atoms in nature
have a mass of 12 u. About 1 percent of carbon atoms have a mass of about 13 u. To find the average, perform the
following calculation:
•
•
0.99 x 12 u + 0.01 x 13 u = 12.01 u
The average mass of a carbon is about 12.01 u.
•
Protons and electrons have electric charge. Opposite charges attract, whereas like charges repel. The proton has a
positive charge, and the electron has a negative charge. The neutron does not have a charge.
8.5 B
•
Scientists have identified over 100 elements. Each element is made of a characteristic type of atom.
All atoms contain a central core called the nucleus. The nucleus contains one or more protons, which are positively
charged particles. Most nuclei also contain neutrons, which are uncharged particles. Neutrons help keep the nucleus
from breaking apart. Surrounding the nucleus are fast-moving electrons, which are very small, negatively charged
particles.
•
The identity of an element is determined by the number of protons in the atomic nucleus. For example, every helium
atom has two protons in its nucleus. Every oxygen atom has eight protons.
•
The number of protons per atom is called the atomic number of the element. Helium has an atomic number of 2.
Oxygen has an atomic number of 8.
•
Atoms of the same element may have different numbers of neutrons in their nuclei. Most helium atoms have two
neutrons, but some have only one neutron.
•
Every atom is electrically neutral. Protons carry the positive charge of the atom, and electrons carry the negative
charge. The number of protons equals the number of electrons.
•
Electrons are organized into energy levels. The first energy level is filled with two electrons, and the second energy
level is filled with eight electrons. For the first 20 elements, eight electrons also fill the third energy level. The
diagram shows the first three elements that have full energy levels: helium, neon, and argon.
•
The electrons in an atom’s outer energy level are called valence electrons. Atoms tend to be most stable when they
have filled outermost energy levels. To reach this stability, atoms gain, lose, or share valence electrons by forming
chemical bonds with other atoms.
Questions?
• The atomic number of oxygen is 8. What do all oxygen
atoms have in common?
• How many possible electrons are in the first and
second energy levels?
• What are valence electrons? How do valence electrons
affect the chemical properties of an element?
• Describe the chemical reaction that occurs between
sodium, whose atoms have 1 valence electron, and
chlorine, whose atoms have 7 valence electrons
Petri Dish Elements
Element
Protons
Neutrons
Electrons
Valence
Electrons
Metal, NonMetal,
Metalloid
Period
Group
Petri Dish Elements
Element
Protons
Neutrons
Electrons
Valence
Electrons
Metal, NonMetal,
Metalloid
Period
Group
8.5C
•
The Periodic Table arranges elements in rows, called periods, and columns, called groups. The order of the
elements is determined by atomic number.
•
The periods grow in size on the table from top to bottom. The first period has only two elements,
hydrogen (atomic number 1) and helium (atomic number 2). The second and third periods each contain
eight elements, and the next two periods each contain 18 elements.
•
The last two periods contain 32 elements. To make the table easier to read, some of these elements are
placed at the bottom of the table.
•
The table is organized so that elements with similar configurations of valence electrons are placed in the
same column, or group. Atoms of elements in Group 1 (including hydrogen, lithium, and sodium) each
have one valence electron. Atoms of elements in Group 17 (including fluorine, chlorine, and bromine) each
have seven valence electrons.
•
Valence electrons help determine the chemical properties of an element. This means that the elements in
a group all have similar chemical properties.
•
The Periodic Table can be used to predict many properties of elements. Metals are located on the left side
and in the center of the table, while nonmetals are clustered on the right side. A staircase-like line divides
the two groups. Elements called metalloids, which have some properties of metals and some properties of
nonmetals, are located along this line.
Teks for Unit 1 and 2
•
(5) Matter and energy. The student knows that matter is composed of atoms and has
chemical and physical properties. The student is expected to:
•
•
Unit 1
(A) describe the structure of atoms, including the masses, electrical charges, and
locations, of protons and neutrons in the nucleus and electrons in the electron cloud;
(B) identify that protons determine an element's identity and valence electrons
determine its chemical properties, including reactivity;
(C) interpret the arrangement of the Periodic Table, including groups and periods, to
explain how properties are used to classify elements;
•
•
•
•
•
•
Unit 2
(D) recognize that chemical formulas are used to identify substances and determine the
number of atoms of each element in chemical formulas containing subscripts;
(E) investigate how evidence of chemical reactions indicate that new substances with
different properties are formed; and
(F) recognize whether a chemical equation containing coefficients is balanced or not and
how that relates to the law of conservation of mass.
Chemistry
Vocabulary,
Unit
1,
part
1
atom: the smallest particle of an element that has all the properties of that element
element: a pure substance, made up of similar atoms, that cannot be broken down by chemical means
nucleus: the center of an atom, which contains protons and neutrons
proton: the subatomic particle in the nucleus that has a positive electric charge
neutron: the subatomic particle in the nucleus that has no electric charge
electron cloud: the region around the nucleus where electrons are found
electron: the negatively charged subatomic particle that exists in a cloud surrounding the nucleus
unified atomic mass unit (u): the unit for measuring the mass of atoms
electric charge: a property of matter that causes it to experience a force near other charged matter
valence electrons: the outermost electrons of an atom, which help determine an element’s chemical
properties
ion: an atom or molecule that has gained or lost one or more electrons
chemical bond: an attractive force between atoms or ions, formed by the sharing or transfer of valence
electrons
Periodic Table: a logical arrangement of the elements into rows and columns; an element’s position in the
Periodic Table can be used to predict its properties
The Periodic Table:
A meeting of the elements
The Periodic Table:
A meeting of the elements
Draw two elements from the element bag on the
teachers desk. Write a minimum of 8 sentences of a
discussion that might occur between the two elements.
Draw two elements from the element bag on the
teachers desk. Write a minimum of 8 sentences of a
discussion that might occur between the two elements.
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