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Periodic Trends Review (1-50)

Total questions: 50

Worksheet time: 44mins

Name
Class
Date
1.
As the elements are considered from top to bottom of group 15 (V A),  which sequence in properties occurs? 
a)
metalloid→metal→nonmetal
b)
nonmetal→metalloid→metal
c)
metal→nonmetal→metalloid
d)
metal→metalloid→nonmetal
2.
In the Periodic Table of the Elements, all of the elements within group 16 (VI A) have the same number of 
a)
neutrons
b)
energy levels
c)
protons
d)
valence electrons
3.
Which group is known as the halogens?
a)
18 (VIII A)
b)
17 (VII A)
c)
1 (I A)
d)
2 (IIV A)
4.
Given the same conditions, which of the following Group 17 (VII A) elements has the highest electron affinity? 
a)
Fluorine
b)
Chlorine
c)
Iodine
d)
Bromine
5.
Which element is a halogen?
a)
Iron
b)
Nitrogen
c)
Iodine
d)
Neon
6.
When fluorine reacts with a Group 1 (IA) metal, it becomes an ion with a charge of
a)
1⁻
b)
2⁺
c)
1⁺
d)
2⁻
7.
In the ground state, how many electrons are in the outermost energy level of each element in Group 17 (VII A)?
a)
8
b)
2
c)
7
d)
5
8.
What is the total number of electrons found in the valence shell of a halogen in the ground state?
a)
1
b)
7
c)
8
d)
2
9.
Which element is in Group 2 (II A) and Period 7 of the Periodic Table?
a)
manganese 
b)
radon
c)
radium
d)
magnesium
10.
An element that has a high ionization energy and tends to be chemically inactive would most likely be
a)
a transition element
b)
a noble gas
c)
an alkali metal
d)
a halogen
11.
In the Periodic Table, the transition elements are found in the 
a)
A groups and Group 18 (VIII A)
b)
B groups, only
c)
A groups, only
d)
B groups and group 8
12.
An atom of the element in Period 2 Group 14 (IV A) is in the ground state. What total number of valence electrons does the atom have?
a)
2
b)
1
c)
4
d)
3
13.
What is the charge of the strontium ion?
a)
2-
b)
1-
c)
1+
d)
2+
14.
Which of the following statements is corrects concerning ions?
a)
Cations form when an atom gains electrons
b)
Cations form when an atom loses electrons
c)
Anions form when an atom gains protons
d)
Anions for when an atom loses protons 
15.
The energy required to remove an electron from gaseous sodium atoms is called 
a)
excitation energy
b)
ionization energy
c)
polarization energy
d)
electrolytic energy 
16.
Which of the following elements, when bound to sulfur attracts electrons less strongly than the sulfur? (least electronegative)
a)
chlorine
b)
cesium
c)
oxygen
d)
fluorine
17.
What term is used to describe an atom's tendency to attract electrons to itself when is is chemically combined with another element?
a)
electronation
b)
electron affinity
c)
electronegativity
d)
electrolysis
18.
Who was responsible for establishing the order in which the elements are presented in the modern periodic table?
a)
Dmitri Mendeleev
b)
Ernest Rutherford
c)
Henry Moseley
d)
Robert Bunsen
19.
A cation is any atom or group of atoms with
a)
a positive charge
b)
no charge
c)
a negative charge
d)
more electrons than the corresponding atoms
20.
The vertical columns of the periodic table are called
a)
groups
b)
rows
c)
periods
d)
transitions
21.
Who first arranged the elements according to atomic mass?
a)
Louis Pasteur
b)
Henry Moseley
c)
John Dalton
d)
Dmitri Mendeleev
22.
The actinides are of greatest interest because of their
a)
abundance
b)
brilliance
c)
reactivity
d)
radioactivity
23.
Choose the atom or ion that has the largest radius
a)
Na
b)
Na+
c)
Both are the same size
24.
Choose the atom or ion that has the largest radius
a)
N
b)
N³⁻
c)
Both are the same size
25.

The ability to attract an electron in a chemical bond

a)

electronegativity

b)

electron affinity

c)

metallic character

d)

ionization energy

26.

The energy it takes to remove an electron from an atom in the gas phase

a)

electron affinity

b)

electronegativity

c)

metallic character

d)

ionization energy

27.

Ionization energy increases

a)

from L to R and from bottom to top

b)

from L to R and from top to bottom

c)

from R to L and from bottom to top

d)

from R to L and from top to bottom

28.

metallic character is greatest

a)

in the top right corner

b)

in the bottom right corner

c)

in the top left corner

d)

in the bottom left corner

29.

Atomic radius decreases from left to right across a period because from left to right there is

a)

increasing number of valence electrons

b)

increasing shielding

c)

increasing effective nuclear charge

d)

increasing number of protons in the nucleus

30.
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)
31.

As atoms of elements in group 16 (VII A) 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

32.

As you move down a group 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 neutrons

33.

The atom with the largest atomic radius in Group 18 (VIII A) is...

a)

Ar

b)

He

c)

Kr

d)

Rn

34.

The element with the highest electronegativity is -

a)

At

b)

F

c)

Cl

d)

Br

35.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
36.

Which atom has the least metallic character?

a)

O

b)

Ba

c)

Co

d)

K

37.

Which atom has the lowest electron affinity?

a)

N

b)

Cl

c)

F

d)

Li

38.

The ionization energy of Na is larger than Cs because...

a)

Na has a greater effective nuclear charge

b)

Na has fewer energy levels and less shielding

c)

Cs has a greater effective nuclear charge than Na

d)

Cs has more valence electrons than Na

39.

Fluorine has a smaller atomic radius than B because...

a)

F has more valence e- than B

b)

F has more shielding than B

c)

F has a larger atomic number than B

d)

F has a greater effective nuclear charge than B

40.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
41.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Nitrogen (N)
b)
Lithium (Li)
c)
Antimony (Sb)
d)
Germanium (Ge)
42.
The vertical columns of the periodic table are called -
a)
groups.
b)
rows.
c)
periods.
d)
transition.
43.
Which orbital block corresponds to transition metals in the periodic table?
a)
s
b)
p
c)
d
d)
f
44.
Which metal on the periodic table is the most reactive?
a)
Cu
b)
Fe
c)
Rb
d)
Fr
45.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
46.

What is the name of family IA

a)

Alkaline Earth Metals

b)

Boron Family

c)

Alkali Metals

d)

Halogen Family

47.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings 
48.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
49.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
50.

As the elements are considered from top to bottom of group 15 (V A), which sequence in properties occurs?

a)

metalloid→metal→nonmetal

b)

nonmetal→metalloid→metal

c)

metal→nonmetal→metalloid

d)

metal→metalloid→nonmetal

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