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WorksheetsChapter 5 Review: The Mole and Periodic Trends
Total questions: 50
Worksheet time: 42mins
Name
Class
Date
1.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
2.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
3.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
4.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
5.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium
c)
francium
d)
cesium
6.
As you move down the periodic table atoms get bigger. This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
7.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
8.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
9.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends.
10.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
11.
Metals are good conductors of heat and electricity.
a)
true
b)
false
12.
The atom with the largest atomic radius in Group 18 is -
a)
Ar
b)
He
c)
Kr
d)
Rn
13.
The element with the lowest electronegativity in Period 3 is -
a)
Na
b)
Cl
c)
Ar
d)
Mg
14.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
15.
An atom's attraction for electrons in a bond is referred to as
a)
electronegativity
b)
ionization energy
c)
electron bond
d)
none of these
16.
What is the energy needed to remove an electron called?
a)
ionization energy
b)
electron energy
c)
electronegativity
d)
electron affinity
17.
The vertical columns of the periodic table are called -
a)
groups.
b)
rows.
c)
periods.
d)
transition.
18.
Which orbital block corresponds to transition metals in the periodic table?
a)
s
b)
p
c)
d
d)
f
19.
A highly reactive group 17 element.
a)
halogen
b)
metalloid
c)
noble gas
d)
alkali metal
20.
An extremely unreactive group 18 element.
a)
halogen
b)
alkali metal
c)
noble gas
d)
alkaline earth metal
21.
Elements that are generally gases or dull brittle solids that are poor conductors of heat and electricity.
a)
noble gas
b)
halogen
c)
nonmetal
d)
metalloids
22.
An element that is solid at room temperature, a good conductor of heat and electricity, and generally is shiny, ductile, and malleable.
a)
metal
b)
nonmetal
c)
metalloid
d)
transition element
23.
How many valence electrons does Hydrogen have?
a)
1
b)
2
c)
3
d)
4
24.
How many valence electrons does Lithium have?
a)
1
b)
2
c)
3
d)
4
25.
How many valence electrons does magnesium have?
a)
1
b)
2
c)
12
d)
24
26.
How many valence electrons does Carbon have?
a)
4
b)
12
c)
6
d)
14
27.
How many valence electrons does Phosphorus have?
a)
31
b)
5
c)
15
d)
4
28.
How many valence electrons does Oxygen have?
a)
8
b)
2
c)
16
d)
6
29.
How many valence electrons does Neon have?
a)
18
b)
8
c)
10
d)
2
30.
How many valence electrons does Sulfur
a)
16
b)
32
c)
6
d)
3
31.
Cations are
a)
positive
b)
negative
c)
on the right side of the periodi table.
d)
nonmetals
32.
Which of the following would produce an anion?
a)
Ca
b)
Al
c)
K
d)
F
33.
Cations are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
34.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
35.
Valence electrons are:
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
36.
Ions are:
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
37.
Which is most likely to form a negative ion?
a)
an element from group 17
b)
a metal
c)
an element from group 1
d)
an element with atoms that have eight valence electrons
38.
Negative ions form when atoms _________ valence electrons.
a)
lose
b)
gain
c)
share
39.
The best definition for a mole provided below is
a)
The SI unit for the mass of something
b)
The SI unit for the amount of a substance
c)
The SI unit for the volume of something
d)
The SI unit for the area of a substance
40.
The number 6.02 x 1023, which is the number of particles found in a mole.
a)
molar mass
b)
mole
c)
Avogadro's number
d)
hydrate
41.
What is the molar mass of copper?
a)
12 g/mol
b)
63.5 g/mol
c)
58.9 g/mol
d)
40.1 g/mol
42.
What is the molar mass of table salt (NaCl)?
a)
116.9 g/mol
b)
35.5 g/mol
c)
23 g/mol
d)
58.4 g/mol
43.
What is the molar mass of fluorine gas?
a)
19 g/mol
b)
38 g/mol
c)
9 g/mol
d)
18 g/mol
44.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
45.
The mass in grams of one mole of any pure substance.
a)
molecular formula
b)
hydrate
c)
mole
d)
molar mass
46.
What was Dmitri Mendeleev's greatest contribution to the history of the periodic table?
a)
He arranged all of the known elements by their atomic number
b)
He realised that there was a pattern of reactivity which repeated every 8 elements
c)
He predicted the existence (and properties) of new elements
d)
He identified the "law of triads" which became the groups
47.
What did Mendeleev use to organize his periodic table?
a)
number of protons
b)
atomic mass
c)
number of electrons
d)
number of neutrons
48.
What did Moseley use to organize his periodic table?
a)
number of protons
b)
atomic mass
c)
number of electrons
d)
number of neutrons
49.
Ionization energy is the amount of energy required to remove the electron that is closest to the nucleus.
a)
True
b)
False
50.
The tendency of an atom to attract electrons is called...
a)
ionization energy
b)
electronegativity
c)
atomic radius
d)
ionic radius
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