Introduction to the Periodic Table
Practice Test
1.
These two elements are liquids at room temperature and pressure.
a.
mercury and oxygen
b.
mercury and bromine
c.
lithium and cesium
d.
silver and nitrogen
2.
These elements have six electrons in their outermost energy levels.
a.
Cr, Mn, and Fe
b.
O, S, and Se
c.
He, Ne, and Ar
d.
Cr, Mo, and W
3.
Which pair of elements would you expect to have similar properties?
a.
F and Ne
b.
Mg and Ti
c.
Si and Ge
d.
Li and Fe
4.
Mendeleev predicted the properties of these two elements, which were unknown at the time.
a.
carbon and silicon
b.
boron and arsenic
c.
gallium and germanium
d.
silicon and aluminum
5.
Mendeleev saw that properties of the elements repeated in an orderly way when he organized them according to ______________.
a.
increasing atomic mass
b.
increasing volume
c.
decreasing atomic number
d.
increasing atomic size
6.
What group of elements was unknown to Mendeleev when he first organized his periodic table?
a.
Group 18, the noble gases
b.
Group 1, the alkali metals
c.
the transition elements
d.
Group 2, the alkaline earth metals
7.
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 3A elements
d.
group 2A elements
8.
In a conductor such as silver, valence electrons are free to move to produce _____________.
a.
nuclei
b.
electrical potential
c.
an electric current
d.
copper atoms
9.
The Lewis electron dot structure for this element contains seven dots.
a.
iodine
b.
francium
c.
manganese
d.
zinc
10.
In general, a metal atom's valence electrons are _____________ the atomic nucleus.
a.
very near
b.
tightly bound to
c.
within
d.
loosely bound to
11.
The properties of the chemical elements in the periodic table occur in ______________.
a.
descending sequence
b.
repeating patterns
c.
ascending sequence
d.
do discernable pattern
12.
Plutonium and americium are ______________.
a.
nonmetals
b.
Noble gases
c.
synthetic elements
d.
metalloids
13.
A transistor may be produced by placing a p-typesemiconductor between two _______________.
a.
molecules
b.
electrons
c.
n-type semiconductors
d.
p-type semiconductors
14.
Except for hydrogen, the elements that are gases at room temperature are ____________.
a.
metals
b.
actinides
c.
metalloids
d.
nonmetals
15.
This scientist arranged some elements in triads based on their atomic masses and other properties.
a.
Newlands
b.
Dobereiner
c.
Mendeleev
d.
Einstein
16.
What is the Group number of the alkali metals?
a.
4
b.
1
c.
3
d.
2
17.
Lanthanides and actinides are known as _________________.
a.
noble gases
b.
halogens
c.
inner transition elements
d.
metalloids
18.
The statement that the physical and chemical properties of the elements repeat in a regular pattern when they are arranged in order of increasing atomic number is known as the ______________.
a.
Group theory
b.
periodic law
c.
Dobereiner's hypothesis
d.
Mendeleev theory
19.
These elements have some physical and chemical properties of metals and other properties of nonmetals.
a.
lanthanides
b.
transition elements
c.
metalloids
d.
actinides
20.
n- and p-type semiconductors may be combined to form _____________.
a.
diodes
b.
transistors
c.
vacuum tubes
d.
cathode-ray tubes
21.
Heavy elements such as seaborgium are created in _____________.
a.
test tubes
b.
particle accelerators
c.
erlenmeyer flasks
d.
earthquakes
22.
Sodium and chlorine react to produce ______________.
a.
sodium chloride
b.
gaseous chlorine
c.
liquid sodium
d.
sodium chlorine
23.
Why was Mendeleev's periodic table widely accepted?
a.
His periodic table listed all of the elements in the correct order.
b.
He predicted the existence and properties of undiscovered elements.
c.
He organized the first 14 known elements.
d.
He was the first to notice a pattern of similar properties among elements.
24.
Noble gases are unreactive because they have a full complement of ________________.
a.
protons
b.
valence electrons
c.
neutrons
d.
inner-level electrons
