The Periodic Table and Periodic Law
Practice Test
1.
Periods are ___________ on the periodic table.
a.
right to left diagonals
b.
left to right diagonals
c.
horizontal rows
d.
vertical columns
2.
How many protons are present in an atom potassium-39?
a.
58
b.
39
c.
20
d.
19
3.
What properties did Rutherford use in the design of the gold foil experiment?
a.
positively charged electrons distributed in a uniform negative charge
b.
alpha particle's negative charge and gold foil's positive charge
c.
alpha particle's negative charge and random distribution of protons
d.
alpha particle's positive charge and electron's negative charge
4.
Which of the following statements concerning hydrogen is false?
a.
All hydrogen isotopes have one electron.
b.
Hydrogen’s electron is not found in the nucleus.
c.
All hydrogen isotopes have one neutron.
d.
All hydrogen isotopes have one proton.
5.
Why are both hydrogen and cesium s-block elements, when hydrogen has one electron and cesium has 55?
a.
Blocks of elements on the periodic table are based only on an element's valence electrons.
b.
All blocks contain at least one element from each period.
c.
They have identical electron configurations.
d.
The s-block includes only the most reactive elements.
6.
In what part of the periodic table would you expect to find an element that emits light when struck by electrons?
a.
actinide series
b.
lanthanide series
c.
group 2A elements
d.
group 3A elements
7.
Which of the following particles has a mass that is almost the same as the mass of a proton?
a.
neutron
b.
positron
c.
electron
d.
beta particle
8.
Atoms with large ionization energy values are __________.
a.
lacking valence electrons
b.
less likely to form positive ions
c.
more likely to form positive ions
d.
most likely to lose their outer electrons
9.
A vapor is a _________.
a.
solid
b.
liquid
c.
condensed state
d.
gas
10.
Which of the following is not a fundamental particle in an atom?
a.
electron
b.
neutron
c.
proton
d.
element
11.
Which group on the periodic table is known as the halogens?
a.
group 7A
b.
group 8A
c.
group 2A
d.
group 1A
12.
Which of the following is the general valence electron configuration for the alkaline earth elements?
a.
ns
2
np
1
b.
ns
1
c.
ns
2
d.
ns
2
np
2
13.
The ionic compound, sodium chloride, is formed from atoms of the elements sodium and chlorine. What happens to the size of each atom when it forms an ion?
a.
Sodium increases in size and chlorine increases in size.
b.
Sodium decreases in size and chlorine increases in size.
c.
Sodium decreases in size and chlorine decreases in size.
d.
Sodium increases in size and chlorine decreases in size.
14.
A material that cannot be broken down further by chemical means is a(n) ________.
a.
element
b.
substance
c.
compound
d.
mixture
15.
A solution of solids is a(n)___________.
a.
filtration
b.
pure metal
c.
heterogeneous mixture
d.
alloy
16.
What is the smallest particle of an element that maintains the properties of the element?
a.
molecule
b.
cation
c.
mixture
d.
atom
17.
The valence orbitals in an atom are the ___________.
a.
innermost orbitals
b.
second energy level
c.
outermost orbitals
d.
d orbitals
18.
A technique that uses the differences in boiling point to separate homogeneous mixtures is _________.
a.
chromatography
b.
distillation
c.
crystallization
d.
filtration
19.
The principle that states each electron occupies the lowest energy orbital available is the ______________.
a.
aufbau principle
b.
exclusion principle
c.
photoelectric principle
d.
uncertainty principle
20.
What type of property is observed when milk sours?
a.
an extensive property
b.
an intensive property
c.
a physical property
d.
a chemical property
