Unit 2 Review
Atomic Structure
1.
The observation of the behavior of a stream of alpha particles bombarded at a thin foil of gold led to
the belief that the atom consisted of _____.
a. electrons orbiting the nucleus with discrete and quantized amounts of energy
b. a positively charged center surrounded by negative electrons
c. negatively charged particles immersed in a sea of positive charge
d. a collection of quarks held together by a strong nuclear force
e. chunky peanut butter and grape jelly
2.
The observation of the unique line spectra of samples of elemental gases led to the belief that the
atom consisted of _____.
a. electrons orbiting the nucleus with discrete and quantized amounts of energy
b. a positively charged center surrounded by negative electrons
c. negatively charged particles immersed in a sea of positive charge
d. a collection of quarks held together by a strong nuclear force
e. chunky peanut butter and grape jelly
3.
If the plum-pudding model of the atom was the correct conception of the atom, then a stream of alpha
particles beamed at a thin gold foil would _____.
a. pass straight through the foil with little to no deflection
b. be absorbed by the atom and not be seen passing through the foil
c. never pass through the atom but instead all be bounced back towards the source
d. mostly pass through the foil but on occasion be bounced back towards the source
4.
What was the evidence from the alpha particle scattering experiment (a.k.a., gold foil experiment)
that led to the conclusion that the mass and the positive charge of an atom are concentrated in a
nucleus?
a. Most of the alpha particles passed through the foil with little to no deflection.
b. An occasional alpha particle bounced back towards the source at an acute angle.
c. The alpha particles were essentially a helium nucleus with positive charge.
d. None of the alpha particles passed through the foil.
5.
Two samples of water are analyzed. One sample contained 16 g of oxygen and 2 g of hydrogen and
the other sample contained 32 g of oxygen and 4 g of hydrogen. This data supports the
a. law of conservation of mass
b. law of definite composition
c. law of multiple proportions
d. law of atomic spectra
For Questions #6 - #11: Match the following historic scientist with the experiment, discovery or
contribution to our understanding of atomic structure. Use the following choices: Ernest Rutherford
(choose A), and Neils Bohr (choose B), J.J. Thompson (choose C), and Dalton (choose D).
6.
Developed the plum-pudding model of the atom.
7.
First person to develop a nuclear model of the atom.
8.
First person credited with providing empirical evidence for the existence of atoms.
9.
Bombarded gold foil with alpha particles and observed scattering.
10.
Suggested that electrons orbit the nucleus in fixed paths with quantized energy levels.
11.
Experimented with cathode rays and discovered the existence of the electron.
12.
All of the following statements are true EXCEPT _____.
a. a proton carries a +1 charge and an electron carries a –1 charge
b. the nucleus of an atom has a negative charge
c. an alpha particle is a helium atom minus its electrons
d. a neutron is an uncharged particle with a mass slightly greater than a proton
e. about 99.9% of an atom’s mass is concentrated in the nucleus
13.
All of the following statements are true EXCEPT _____.
a. all atoms of a given element have the same mass number
b. for any neutral element, the number of electrons is equal to the number of protons
c. the mass number is the sum of the number of protons and neutrons
d. isotopes of atoms contain the same number of protons but a different number of neutrons
e. the atomic number equals the number of protons in an atom
Isotopes, Isotope Notation, Protons, Neutrons, Electrons
14.
The charged particles of the atom are _____. Bubble in all that apply.
a. proton
b. neutron
c. electron
15.
The _____ comprise most of the mass of an atom.
a. protons only
b. neutrons only
c. electrons only
d. protons and neutrons
e. protons and electrons
16.
The atomic number of an element refers to the number of _____ in an atom of that element.
a. protons
b. neutrons
c. electrons
d. protons and neutrons
17.
The mass number of an atom refers to the number of _____ in an atom of that element.
a. protons
b. neutrons
c. electrons
d. protons and neutrons
18.
Isotopes are two atoms of the same element have the same number of ______ and a different number
of ______.
a. electrons, protons b. protons, electrons c. neutrons, protons
d. protons, neutrons
19.
Which of the following pairs of atoms are isotopes?
a. An atom of aluminum with 14 neutrons and an atom of silicon with 14 neutrons.
b. An atom of silicon with 13 protons and an atom of aluminum with 13 protons.
c. An atom of aluminum with 13 protons and an atom of silicon with 14 protons.
d. An atom of silicon with 14 neutrons and an atom of silicon with 15 neutrons.
20.
What is the identity of 24 X ?
a. magnesium (Mg) b. vanadium (V)
d. rubidium (Rb)
e. antimony (Sb)
21.
51
Which of the
! following atoms contains the smallest number protons?
a. neon-20
22.
c. chromium (Cr)
b. magnesium-23
c. sodium-23
d. silicon-27
Which of the following atoms contains the smallest number neutrons?
a. zinc-64
b. coper-63
c. nickel-58
d. manganese-58
23.
Which description most accurately describes mercury-224?
a. number of protons = 80, atomic number = 224
b. mass number = 80, number of neutrons = 144
c. atomic number = 80, mass number = 144
d. mass number = 80, atomic number = 224
e. number of protons = 80, number of neutrons = 144
24.
Which two atoms below have the same number of protons?
20
10
a.
23
11
Na
and
c.
22
11
Na
and! 12 Mg!
e.
20
10
!
!
25.
23
11
!
Na ,
22
11
27
14
Na ,
Si
b.
23
12
and
23
11
Na
d.
12
and
27
14
Si
!
20
10
!
Mg
23 !
Mg
!
a.
23
11
Na
and
c.
22
11
Na
and! 12 Mg!
e.
20
10
Ne
!
22
11
Ne ,
23
11
Na
!
23
and
!
Mg ,
23
12
23
11
Na
!
!
Na ,
22
11
27
14
Na ,
Si
b.
23
12
and
23
11
Na
d.
12
and
27
14
Si
!
Mg
23 !
Mg
!
26.
How many electrons, protons, and neutrons are found in a Cl- ion formed from Cl-35?
!electrons, 16 protons, 19 neutrons
!
a. 17
b. 17!electrons, 17 protons, 18 neutrons
c. 18 electrons, 18 protons, 18 neutrons
d. 18 electrons, 17 protons, 18 neutrons
!electrons, 18 protons, 17 neutrons
e. 18
27.
How many electrons, protons, and neutrons are found in a Mg2+ ion formed from Mg-24?
a. 12 electrons, 10 protons, 14 neutrons
b. 12 electrons, 10 protons, 12 neutrons
c. 12 electrons, 12 protons, 24 neutrons
d. 14 electrons, 12 protons, 24 neutrons
e. 14 electrons, 12 protons, 12 neutrons
28.
Which two of the ions below have the same number of electrons?
!
58
25
a.
64
30
c.
63
29
e.
!
!
!
Na
!
!
!
23
11
Mg ,
Na
23
and
23
12
Which two atoms below have the same number of neutrons?
!
!
Ne
!
22
11
Ne ,
29.
Zn 2 +
and
70
31
Cu 2 +
!2 +
63
Cu
29
!
and
64
30
and
Mn 5 + ,
58
28
Ni 2 + ,
63
29
Cu 2 + ,
64
30
Zn 2 + ,
Ga 3 +
b.
58
25
Mn 5 +
Zn 2 +
! 2+
63
29 Cu
d.
63
29
Cu 2 +
!
!
!
!
and
and
70
31
58
28
70
31
Ni 2 +
Ga 3 +
!
Which of these particles has 10 electrons? Bubble in all that apply.
!
!
a. F- !
b. Ne
c. Mg2+
!
Ga 3 +
d. Si4-
Periodic Table and Periodic Law
30.
Based on their location on the periodic table, oxygen (O) and selenium (Se) have
a. the same number of neutrons
b. similar atomic masses
c. similar properties
d. the same number of electrons
31.
Which element can be found in the third group and the fourth period of the periodic table?
a. Be
b. Ga
c. Sc
d. Si
32.
Which one of the following elements is a metalloid?
a. aluminum (Al)
b. radon (Rn)
c. silicon (Si)
d. tin (Sn)
For Questions #33 - #45: Classify the following elements as alkali metals (AM), alkali earth metals
(AEM), transition metals (TM), halogens (H), or noble gases.
33.
10
Ne:
a. AM
b. AEM
c. TM
d. H
e. NG
34.
11
Na:
a. AM
b. AEM
c. TM
d. H
e. NG
35.
17Cl:
a. AM
b. AEM
c. TM
d. H
e. NG
36.
20
Ca:
a. AM
b. AEM
c. TM
d. H
e. NG
Fe:
a. AM
b. AEM
c. TM
d. H
e. NG
Kr:
37.
26
38.
36
a. AM
b. AEM
c. TM
d. H
e. NG
39.
47Ag:
a. AM
b. AEM
c. TM
d. H
e. NG
40.
53
I:
a. AM
b. AEM
c. TM
d. H
e. NG
41.
12
Mg:
a. AM
b. AEM
c. TM
d. H
e. NG
42.
24
Cr:
a. AM
b. AEM
c. TM
d. H
e. NG
43.
35Br:
a. AM
b. AEM
c. TM
d. H
e. NG
44.
86
Rn:
a. AM
b. AEM
c. TM
d. H
e. NG
45.
10
Ne:
a. AM
b. AEM
c. TM
d. H
e. NG
The element calcium is often represented on a periodic table by the information
shown at the right. Use this information to answer the next two questions.
46. The number 20 as shown in the graphic represents the _____ for calcium.
a. atomic number
b. mass number
c. number of electrons
d. average atomic mass
e. number of neutrons
47.
The number 40.078 as shown in the graphic represents the _____ for calcium.
a. atomic number
b. mass number
c. number of electrons
d. average atomic mass
e. number of neutrons
48.
There are two isotopes of the element fluorine: fluorine-18 and fluorine-19. Which one of the
isotopes is most abundant in nature?
a. fluorine-18
b. fluorine-19
c. There is no way to make such a judgment.
49.
Copper has two isotopes, copper-63 with an atomic mass of 62.94 amu and copper-65 with an atomic
mass of 64.93 amu. Calculate the average atomic mass for copper given the percent abundance of
copper-63 is 69.17% and the percent abundance of copper-65 is 30.83%.
a. 31.78 amu
b. 64.00 amu
c. 63.55 amu
d. 63.93 amu
Consider the diagram of the periodic table found below at the right. Match the shaded regions (and their
associated letters) to the names given to the following regions of the table of elements.
50.
Non-metals
51.
Noble Gases
52.
Metals
53.
Metalloids
54.
How many nonmetals, metalloids, and metals are in group 14?
a. 0 nonmetals, 3 metalloids, and 2 metals
b. 1 nonmetal, 2 metalloids, and 2 metals
c. 2 nonmetals, 2 metalloids, and 1 metal
d. 2 nonmetals, 1 metalloid, and 2 metals
e. 3 nonmetals, 0 metalloids, and 2 metals
Naming and Formula Writing; Ion Charges
55.
Ionic compounds are compounds that consist of _____. Bubble in all that apply.
a. oppositely charged ions
b. two metallic elements
c. liked charged ions
d. two non-metallic elements
56.
Which of the following are ionic compounds? Bubble in all that apply.
a. KCl
b. CO2
c. BaO
d. CCl4
57.
Which of the following are molecular compounds? Bubble in all that apply.
a. KCl
b. CO2
c. BaO
d. CCl4
58.
Identify the ions and their charges in Fe2O3.
a. Fe+, O3b. Fe2+, O33+
3d. Fe2 , O2
e. Fe26+, O36-
c. Fe3+, O2-
59. Identify the ions and their charges in Al2(SO4)3.
a. Al+, SO43b. Al3+, SO42c. Al3+, SO433+
26+
6d. Al2 , SO4
e. Al2 , SO4
60.
What are the values for x and y, respectively, in NaxHyPO4? (This assumes that a 1 can be written in
the formula if the x or y value is 1.)
a. 1 and 2
b. 2 and 1
c. 1 and 3
d. 2 and 2
e. 1 and 1
61.
What are the values for x and y, respectively, in Alx(SO4)y? (This assumes that a 1 can be written in
the formula if the x or y value is 1.)
a. 1 and 1
b. 1 and 2
c. 1 and 3
d. 2 and 3
e. 3 and 2
62.
Which of the following are acids? Bubble in all that apply.
a. Na2SO4
b. H2SO4
c. BH3
d. H2C2 O4
Process/Laboratory
At the beginning of the unit, Honors Chemistry students
conducted the online Alpha Particle Scattering Simulation.
To help you remember the activity, a screenshot is shown at
the right. The next two questions are based upon this
activity.
63.
One of the procedural steps in the activity involved
changing the number of protons and neutrons in the
nucleus. Upon changing the value, the affect of the
change on the path of alpha particles was observed. It
was found that changing the number of neutrons had
no affect on the path. Yet changing the number of
protons affected the path. More alpha particles were
scattered at larger angles when the number of protons
was increased.
What single conclusion could be made based upon
this observation?
a. Neutrons are not located in the nucleus of an atom;
they must be located elsewhere in the atom.
b. Alpha particles do not contain any neutrons since altering the neutrons of the atom has no affect.
c. Alpha particles scatter because of a charge interaction; the more charge, the more scattering.
d. Alpha particles scatter when they bounce off massive objects; the more mass, the more scattering.
64.
During the simulation, many alpha particles passed by the atom with little to no interaction. This is
shown in the screenshot above. Which statement is consistent with this observation?
a. Orbiting electrons attract alpha particles; this influence makes the path more straight.
b. The affect of the nucleus upon the alpha particles is less at greater distances from the nucleus.
c. Alpha particles naturally spiral through space; the nucleus tends to straighten them out.
d. Alpha particles are attracted to the nucleus; this attraction is less at greater distances