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Periodic Trends & Electron Configuration Review

Total questions: 74

Worksheet time: 2hrs 7mins

Name
Class
Date
1.

Horizontal row in the periodic table

a)

group

b)

valence electrons

c)

period

d)

family

2.

subatomic particles that are transferred to form positive and negative ions

a)

electrons

b)

protons

c)

neutrons

3.

type of element that is a good conductor of energy (ex. heat , electricity)

a)

nonmetal

b)

metalloid

c)

metal

d)

all elements

4.

ability of an atom to attract electrons when the atom is in a compound

a)

electronegativity

b)

ionization energy

c)

atomic radius

d)

periodic law

5.

an ion with a positive charge

a)

anion

b)

cation

c)

nonmetals

d)

halogens

6.

the amount of energy needed to remove an electron

a)

electronegativity

b)

ionization energy

c)

periodic energy

d)

atomic energy

7.

Which statement is true about electronegativity

a)

electronegativity is the ability of an anion to attract another anion

b)

electronegativity generally increases as you move from top to bottom within a group

c)

electronegativity generally is higher for metals than for non metals

d)

electronegativity generally increases from left to right across a period

8.

Which of the following will have a larger radius than Zinc (Zn)?

a)

Gallium (Ga)

b)

Aluminum (Al)

c)

Magnesium (Mg)

d)

Strontium (Sr)

9.

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)

10.
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
11.
Elements on the far right side of the periodic table are classified as nonmetals.
a)
true
b)
false
12.

Which atom has the largest atomic radius?

a)

potassium (K)

b)

rubidium (Rb)

c)

francium (Fr)

d)

cesium (Ce)

13.

Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?

a)

fluorine (F)

b)

chlorine (Cl)

c)

bromine (Br)

d)

iodine (I)

14.

Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?

a)

beryllium, Be

b)

potassium, K

c)

titanium, Ti

d)

yttrium, Y

15.

Each period in the periodic table corresponds to a(n)

a)

principle energy level

b)

energy sublevel

c)

orbital

d)

suborbital

16.

Of the following elements which is a non metal

a)

Pt

b)

V

c)

Li

d)

Kr

17.

Which statement is true about electronegativity

a)

electronegativity is the ability of an anion to attract another anion

b)

electronegativity generally increases as you move from top to bottom within a group

c)

electronegativity generally is higher for metals than for non metals

d)

electronegativity generally increases from left to right across a period

18.

For groups 13 through 18, the number of valence electrons is equal to the group number

a)

plus 1

b)

plus the period number

c)

minus the period number

d)

minus 10

19.

Which element has the highest electronegativity?

a)

cesium (Cs)

b)

helium (He)

c)

fluorine (F)

d)

calcium (Ca)

20.

How does atomic radius change from left to right across a period in the periodic table

a)

it tends to decrease

b)

it tends to increase

c)

it first increases, then decreases

d)

it first decreases, then increases

21.
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
22.
Elements on the far right side of the periodic table are classified as nonmetals.
a)
true
b)
false
23.

Which has the greater electronegativity:

H or F?

a)

H

b)

F

24.

Which atom has the largest atomic radius?

a)

potassium (K)

b)

rubidium (Rb)

c)

francium (Fr)

d)

cesium (Ce)

25.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
26.

Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?

a)

fluorine (F)

b)

chlorine (Cl)

c)

bromine (Br)

d)

iodine (I)

27.

All elements found on the left side of the Periodic Table of the Elements have what properties in common?

a)

They conduct heat and electricity

b)

They are all gases

c)

They are brittle and dull

d)

They are radioactive

28.

Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?

a)

beryllium, Be

b)

potassium, K

c)

titanium, Ti

d)

yttrium, Y

29.

The number of valence electrons in an element affects the reactivity of that element. Which element listed has the fewest valence electrons?

a)

beryllium (Be)

b)

sodium (Na)

c)

oxygen (O)

d)

neon (Ne)

30.

According to the Periodic Table of the Elements, which set of elements has similar properties?

a)

H, C, I

b)

He, H, Al

c)

He, Ne, Ar

d)

Na, Ca, Al

31.

Which element has 2 valence electrons?

a)

cesium (Cs)

b)

magnesium (Mg)

c)

boron (B)

d)

argon (Ar)

32.

How many valance electrons does Iodine (I) have?

a)

6

b)

16

c)

7

d)

17

33.

How many periods are on the periodic table of elements

a)

6

b)

7

c)

8

d)

9

34.
What do you call the vertical columns on the periodic table?
a)
Groups
b)
Periods
c)
Rows
d)
Trends
35.
What is another name for group?
a)
Family
b)
Law
c)
Period
d)
Repetition
36.
Which type of element is malleable?
a)
Metal
b)
Nonmetal
c)
Metalloid
37.
Which type of element is in-between a metal and a nonmetal?
a)
Group
b)
Family
c)
Metalloid
d)
Period
38.
Which type of element is dull (not shiny)?
a)
Metal
b)
Nonmetal
c)
Metalloid
39.

Which type of element is boron (B)?

a)

Metal

b)

Nonmetal

c)

Metalloid

40.
What are the electrons in the outer most energy level called?
a)
Halogens
b)
Metals
c)
Oxidation Number
d)
Valence Electrons
41.

As you move across the periodic table atoms tend to get smaller because, ______________.

a)

the atoms have more mass.

b)

the atoms have more protons and increased electron shielding.

c)

the atoms have more protons and electrons are added to the same energy level.

d)

the atoms have more protons, electrons, and increased electron shielding.

42.

The most dominant factor affecting the attraction between the outermost electrons and the nucleus is the

a)

distance between the nucleus and outermost electrons.

b)

none of these are correct.

c)

total number of electrons.

d)

number of protons/ nuclear charge.

43.

What kind of element can conduct electricity, but be brittle (not malleable)?

a)

some nonmetals

b)

metalloids

c)

some metals

d)

all nonmetals

44.
In what section would Noble Gases be found?
a)
white
b)
yellow
c)
blue
d)
red
45.

Which color on the image of the periodic table corresponds with the transition metals.

a)

red

b)

black

c)

blue

d)

orange

46.

Which color on the image of the periodic table corresponds with the metalloids.

a)

bright yellow

b)

gold

c)

teal

d)

light blue

47.

What atom matches this electron configuration?

1s2 2s2 2p6 3s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

48.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
49.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
50.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
51.

What is this element?

1s22s22p63s23p64s23d104p6

a)

Argon

b)

Krypton

c)

Selenium

d)

Bromide

52.

What is the shorthand electron configuration for Sulfur atom?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p3

53.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
54.

Which element is pictured?

a)

neon - 1s22s22p6

b)

fluorine - 1s22s22p5

c)

magnesium - 1s22s22p63s2

d)

argon - 1s22s22p63s23p6

55.

Identify the element in Period 5 that has 1 valence electron?

a)

Rb

b)

Nb

c)

Ag

d)

Sb

56.

What element in Period 4 has 5 valence electrons?

a)

Zr

b)

As

c)

V

d)

Sb

57.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
58.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
59.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
60.

Primary energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

61.

Which element is depicted from this orbital diagram

a)

Fluorine - 1s22s22p5

b)

Neon - 1s22s22p6

c)

Chlorine - 1s22s22p63s23p5

d)

Argon - 1s22s22p63s23p6

62.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
63.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
64.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
65.

Which of the following sub-levels is correctly designated?

a)

1p5

b)

3f9

c)

2p6

d)

3d11

66.

What is the difference in a 1s orbital and a 2s orbital?

a)

The shape of the orbital

b)

The size of the orbital

c)

The number of electrons it can hold

d)

None of the above

67.
If distance remains the same, as the number of protons increases, the force of attraction
a)
remains the same
b)
increases
c)
decreases
d)
is divided by 1/2
68.

Why does Ca have a larger radius than Se?

a)

It has more energy levels

b)

It has fewer energy levels

c)

It has a more effective nuclear charge

d)

It has a less effective nuclear charge

69.

Why is S smaller than Te?

a)

It has more energy levels.

b)

It has fewer energy levels.

c)

It has a more effective nuclear charge.

d)

It has a less effective nuclear charge.

70.

What is effective nuclear charge?

a)

The charge that effects the mass of the atom.

b)

The charge that the protons feel from the rest of the atom.

c)

The charge felt by the valence electrons.

d)

The charge felt by the core electrons.

71.

In the following configuration, which electrons are the core electrons? 1s2 2s2 2p6 3s2 3p4

a)

1s2 2s2 2p6

b)

3s2 3p4

c)

1s2 2s2

d)

2s2 2p6 3s2 3p4

72.

What electron configuration matches an oxygen atom?

a)

[Ar]4s23d104p5

b)

[He]2s22p4

c)

1s22s22p6

d)

[Ar] 4s23d1

73.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

74.

How many electrons should Boron have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

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