Introduction to the Periodic Table
Practice Test
1.
What group of elements was unknown to Mendeleev when he first organized his periodic table?
a.
Group 1, the alkali metals
b.
Group 18, the noble gases
c.
the transition elements
d.
Group 2, the alkaline earth metals
2.
This scientist arranged some elements in triads based on their atomic masses and other properties.
a.
Newlands
b.
Einstein
c.
Dobereiner
d.
Mendeleev
3.
Heavy elements such as seaborgium are created in _____________.
a.
erlenmeyer flasks
b.
earthquakes
c.
particle accelerators
d.
test tubes
4.
Lanthanides and actinides are known as _________________.
a.
noble gases
b.
halogens
c.
inner transition elements
d.
metalloids
5.
Sodium and chlorine react to produce ______________.
a.
liquid sodium
b.
sodium chloride
c.
gaseous chlorine
d.
sodium chlorine
6.
Mendeleev predicted the properties of these two elements, which were unknown at the time.
a.
gallium and germanium
b.
carbon and silicon
c.
boron and arsenic
d.
silicon and aluminum
7.
Why was Mendeleev's periodic table widely accepted?
a.
He organized the first 14 known elements.
b.
He was the first to notice a pattern of similar properties among elements.
c.
He predicted the existence and properties of undiscovered elements.
d.
His periodic table listed all of the elements in the correct order.
8.
Which element is NOT suitable to dope silicon to produce an n-type semiconductor?
a.
carbon
b.
arsenic
c.
phosphorus
d.
antimony
9.
These elements have some physical and chemical properties of metals and other properties of nonmetals.
a.
actinides
b.
lanthanides
c.
transition elements
d.
metalloids
10.
Plutonium and americium are ______________.
a.
synthetic elements
b.
nonmetals
c.
metalloids
d.
Noble gases
11.
A transistor may be produced by placing a p-typesemiconductor between two _______________.
a.
molecules
b.
electrons
c.
n-type semiconductors
d.
p-type semiconductors
12.
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
13.
Which pair of elements would you expect to have similar properties?
a.
Li and Fe
b.
Mg and Ti
c.
F and Ne
d.
Si and Ge
14.
The Lewis electron dot structure for this element contains seven dots.
a.
manganese
b.
iodine
c.
francium
d.
zinc
15.
The properties of the chemical elements in the periodic table occur in ______________.
a.
do discernable pattern
b.
repeating patterns
c.
descending sequence
d.
ascending sequence
16.
In what part of the periodic table would you expect to find an element that emits light when struck by electrons?
a.
lanthanide series
b.
group 3A elements
c.
actinide series
d.
group 2A elements
17.
In general, a metal atom's valence electrons are _____________ the atomic nucleus.
a.
within
b.
tightly bound to
c.
very near
d.
loosely bound to
18.
These two elements are liquids at room temperature and pressure.
a.
lithium and cesium
b.
mercury and bromine
c.
silver and nitrogen
d.
mercury and oxygen
19.
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.
Dobereiner's hypothesis
c.
Mendeleev theory
d.
periodic law
20.
n- and p-type semiconductors may be combined to form _____________.
a.
diodes
b.
cathode-ray tubes
c.
vacuum tubes
d.
transistors
21.
This element is a halogen.
a.
bromine
b.
carbon
c.
oxygen
d.
nitrogen
22.
These elements have six electrons in their outermost energy levels.
a.
O, S, and Se
b.
Cr, Mo, and W
c.
Cr, Mn, and Fe
d.
He, Ne, and Ar
23.
Noble gases are unreactive because they have a full complement of ________________.
a.
inner-level electrons
b.
neutrons
c.
valence electrons
d.
protons
24.
What is the Group number of the alkali metals?
a.
4
b.
3
c.
2
d.
1
