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Electron and Periodic Trend Review

Total questions: 75

Worksheet time: 38mins

Name
Class
Date
1.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

2.

What is one-half the distance between the nuclei of identical atoms that are bonded together?

a)

atomic radius

b)

atomic diameter

c)

atomic width

d)

atomic length

3.

What is a positively-charged ion which forms when an atom loses electrons?

a)

atom

b)

ion

c)

cation

d)

anion

4.

What is a negatively-charged ion which forms when an atom gains electrons?

a)

cation

b)

anion

c)

electron

d)

ion

5.

What is a vertical (up and down) column in the periodic table?

a)

group or family

b)

period

c)

periodic law

d)

octet rule

6.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
7.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
8.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
9.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
10.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
11.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
12.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
13.

Ions are formed when atoms gain or lose ___.

a)

electrons

b)

protons

c)

neutrons

d)

atomic mass

14.

What property is being measured in this diagram?

a)

Density

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

15.

If a potassium atom lost one electron, what would be the symbol for that ion?

a)
b)
c)
d)
16.

What type of elements are poor conductors of heat and electricity?

a)

transition metals

b)

inner transition metals

c)

metals

d)

nonmetals

17.

What type of elements are malleable and ductile?

a)

noble gases

b)

nonmetals

c)

metals

d)

halogens

18.

Select the sequence that correctly orders from smallest to largest atomic radius

a)

Sn, Y, Ru

b)

Cu, Ga, Br

c)

Al, S, Na

d)

F, N, Li

19.

Select the sequence of increasing electronegativity.

a)

Sn, Ag, I

b)

I, Sn, Ag

c)

Ag, Sn, I

d)

Sn, I, Ag

20.

What group contains elements with 7 valence electrons

a)

Noble Gasses

b)

Alkali Earth Metals

c)

Halogens

d)

Transition Metals

21.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
22.
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.
23.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
24.
Magnesium (Mg) is part of the _ family.
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
25.
How many valence electrons does an alkaline earth metal have? 
a)
1
b)
2
c)
7
d)
8
26.

F and Cl.


Which has the greatest atomic radius? Justify your answer using claim, evidence, and reasoning.

4 lines
27.

In the process of ionization, what is the relationship between the second ionization energy (I2) and the third ionization energy (I3)?

a)

I2 > I3

b)

I2 < I3

c)

I2 = I3

d)

There is no way to predict this relationship.

28.

Consider the group 1A elements sodium (period 3), potassium (period 4), and rubidium (period 5). What would you predict about the ionization energies of these elements?

a)

Na < K < Rb

b)

Na > K > Rb

c)

Rb < Na < K

d)

Na = K = Rb

29.

Which element in period 4 has the highest electronegativity?

a)

potassium

b)

calcium

c)

copper

d)

bromine

30.

Which of these elements in group 1A has the largest atomic radius?

a)

cesium

b)

rubidium

c)

potassium

d)

sodium

31.

Consider the group 1A element sodium (atomic number 11), the group 3A element aluminum (atomic number 13), and the group 7A element chlorine (atomic number 17). These elements are in period 3. How are the first ionization energies of these elements related?

a)

sodium > aluminum > chlorine

b)

sodium < aluminum < chlorine

c)

sodium < chlorine < aluminum

d)

sodium > chlorine > aluminum

32.

The sodium atom loses an electron to form a sodium ion (Na+). Which statement is correct with respect to its atomic radius?

a)

The sodium ion has a larger radius than the atom.

b)

The sodium ion has a smaller radius than the atom.

c)

The sodium ion and the sodium atom radii are the same size.

d)

The sodium ion has twice the radius of the sodium atom.

33.

As you move left to right across a period, ionization energy

a)

increases

b)

decreases

c)

says the same

34.

Which of the following has the largest electronegativity value?

a)

neon

b)

fluorine

c)

carbon

d)

lithium

35.

Why does radius increase as you move down a group?

a)

protons are being added

b)

ionization energy is increasing

c)

protons are getting weaker

d)

energy levels are being added

36.

What are the elements in the center (d block) of the periodic table?

a)

Inner Transition Metals

b)

Alkali Metals

c)

Transition Metals

d)

Alkaline Earth Metals

37.

What are the elements in the two rows below the periodic table (f block)?

a)

Inner Transition Metals

b)

Alkali Metals

c)

Transition Metals

d)

Alkaline Earth Metals

38.

Which are great conductors?

a)

Metals

b)

Nonmetals

c)

Metalloids

39.

Which are used as semiconductors?

a)

Metals

b)

Nonmetals

c)

Metalloids

40.

Which are poor conductors, dull, and gases at room temperature?

a)

Metals

b)

Nonmetals

c)

Metalloids

41.

Atomic radius _______ down a group and _______ across a period.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

42.

Ionization energy_______ down a group and _______ across a period.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

43.

Electronegativity_______ down a group and _______ across a period.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

44.

Who organized the first periodic table?

a)

Mendeleev

b)

Moseley

c)

Mozart

d)

Lavosier

45.

Identify the period and group of the element that has the electron configuration 1s2 2s2 2p6 3s2 3p3.

a)

Period 2 group 12

b)

Period 3 group 11

c)

Period 3 group 13

d)

Period 3 group 15

46.

What is the electron configuration of the element in period 3, group 16?

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3d10 3p4

c)

1s2 2s2 2p6 3s2 3p4

d)

1s2 2s2 2p6 3s2 3p2

47.

Which of the following is a d block element

a)

Be

b)

Si

c)

Ni

d)

Th

48.
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
49.
How did Mendeleev arrange the elements?
a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
50.

How many valance electrons does iodine have?

a)

6

b)

16

c)

7

d)

17

51.
Put these in order of increasing electronegativity:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
52.

Atomic size

a)

increases moving down a group and increases moving left to right on a period

b)

decrease moving down a group and decreases moving left to right on a period

c)

increases moving down a group and decreases moving left to right on a period

d)

decreases moving down a group and increases moving left to right on a period

53.

Ionization energy

a)

increases moving down a group and increases moving left to right on a period

b)

decrease moving down a group and decreases moving left to right on a period

c)

increases moving down a group and decreases moving left to right on a period

d)

decreases moving down a group and increases moving left to right on a period

54.
What is the correct electron configuration for Cs1+
a)
[Kr]5s24d105p66s1
b)
[Xe]6s2
c)
[Xe]6s1
d)
[Kr]5s24d105p6
55.

Which is larger:

P or P-3 ?

a)

P because it is the neutral atom.

b)

P-3 because it lost 3 electrons.

c)

P-3 because it gained 3 electrons.

d)

They are the same size since they are both P.

56.

Which is the smaller atom: Mg or Mg+2?

a)

Mg because it gains an energy level since it gains 2 electrons.

b)

Mg due to extra electron repulsion created by gaining 2 electrons.

c)

Mg+2 because of extra electron repulsion created by gaining 2 electrons.

d)

Mg+2 because it loses an energy level since it loses 2 electrons.

57.

When an atom gains an electron, the size of atom

a)

will increase

b)

will decrease

c)

will not change

58.

When an atom loses an electron the size of atom

a)

will increase

b)

will decrease

c)

will not change

59.

Which species has the larger radius?

a)

Cl

b)

Cl-

60.

Which species has the larger radius?

a)

Na

b)

Na+

61.

______arranged elements in a periodic table according to the increasing order of atomic number

a)

John Newlands

b)

Dimitri Mendeleev

c)

Henry Mosely

d)

Lothar Mayer

62.

  Why were there blank spaces left in Mendeleev's periodic table?                                             

a)

 He didn't know what to put there.

b)

  Undiscovered elements not yet known.

c)

Multiple elements could have fit

d)

He forgot to add the elements in

63.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
64.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
65.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
66.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
67.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
68.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
69.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
70.
What does Hund's rule states ?
a)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
71.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)

states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electrons have opposite spins

c)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
72.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
73.

What is the maximum number of electrons that an s orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

74.

How many electrons can the p sublevel hold?

a)
8
b)

6

c)
2
d)
4
75.

Which electron configuration belongs to a Chloride (Cl-) ion?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

d)

1s2 2s2 2p6 3p7

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