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Periodic Table and Trends Review

Total questions: 88

Worksheet time: 51mins

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.

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

a)

principle energy level

b)

energy sublevel

c)

orbital

d)

suborbital

8.

Of the following elements which is a non metal

a)

Pt

b)

V

c)

Li

d)

Kr

9.

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

10.

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

11.

Which element has the highest electronegativity?

a)

cesium (Cs)

b)

helium (He)

c)

fluorine (F)

d)

calcium (Ca)

12.

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

13.

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

a)

Gallium (Ga)

b)

Aluminum (Al)

c)

Magnesium (Mg)

d)

Strontium (Sr)

14.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

15.

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)

16.
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
17.
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.
18.
Elements on the far right side of the periodic table are classified as nonmetals.
a)
true
b)
false
19.

Which has the greater electronegativity:

H or F?

a)

H

b)

F

20.

Which atom has the largest atomic radius?

a)

potassium (K)

b)

rubidium (Rb)

c)

francium (Fr)

d)

cesium (Ce)

21.
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.
22.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
23.

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)

24.

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

25.

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

26.

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)

27.

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

28.
What is the family name of this group of elements? 
a)
Alkali metals 
b)
Halogens 
c)
Noble Gases 
d)
Alkali Earth Metals 
29.

Which element has 2 valence electrons?

a)

cesium (Cs)

b)

magnesium (Mg)

c)

boron (B)

d)

argon (Ar)

30.

How many valance electrons does Iodine (I) have?

a)

6

b)

16

c)

7

d)

17

31.

Metals have the largest -

a)

atomic radius and electronegativity

b)

electronegativity and ionization energy

c)

atomic radius only

d)

ionization energy and atomic radius

32.

How many periods are on the periodic table of elements

a)

6

b)

7

c)

8

d)

9

33.
What do you call the vertical columns on the periodic table?
a)
Groups
b)
Periods
c)
Rows
d)
Trends
34.
What is another name for group?
a)
Family
b)
Law
c)
Period
d)
Repetition
35.
Which type of element is malleable?
a)
Metal
b)
Nonmetal
c)
Metalloid
36.
Which type of element is in-between a metal and a nonmetal?
a)
Group
b)
Family
c)
Metalloid
d)
Period
37.
Which type of element is dull (not shiny)?
a)
Metal
b)
Nonmetal
c)
Metalloid
38.

Which of the following would be malleable and ductile?

a)

Carbon (C)

b)

Sulfur (S)

c)

Chlorine (Cl)

d)

Iron (Fe)

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.

Chlorine has 17 electrons. According to the modern atomic theory, how many electrons are found in n = 2, the second energy level?

a)

7

b)

2

c)

8

d)

17

45.

According to the Bohr model, what may happen when an atom gains energy?

a)

The electron moves to a higher energy level.

b)

The electron moves to a lower energy level.

46.
In what section would Noble Gases be found?
a)
white
b)
yellow
c)
blue
d)
red
47.

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

a)

red

b)

black

c)

blue

d)

orange

48.

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

a)

red

b)

black

c)

blue

d)

orange

49.

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

a)

bright yellow

b)

gold

c)

teal

d)

light blue

50.

What atom matches this electron configuration?

1s2 2s2 2p6 3s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

51.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
52.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
53.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
54.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
55.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
56.

What is this element?

1s22s22p63s23p64s23d104p6

a)

Argon

b)

Krypton

c)

Selenium

d)

Bromide

57.

What is the shorthand electron configuration for Sulfur atom?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p3

58.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
59.

Which element is pictured?

a)

neon - 1s22s22p6

b)

fluorine - 1s22s22p5

c)

magnesium - 1s22s22p63s2

d)

argon - 1s22s22p63s23p6

60.

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

a)

Rb

b)

Nb

c)

Ag

d)

Sb

61.

What element in Period 4 has 5 valence electrons?

a)

Zr

b)

As

c)

V

d)

Sb

62.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
63.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
64.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
65.

Primary energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

66.

Which element is depicted from this orbital diagram

a)

Fluorine - 1s22s22p5

b)

Neon - 1s22s22p6

c)

Chlorine - 1s22s22p63s23p5

d)

Argon - 1s22s22p63s23p6

67.

Which orbital has the least amount of energy?

a)

p orbital

b)

d orbital

c)

s orbital

d)

What is an orbital?

68.
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.
69.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
70.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
71.
What is the shape of a p orbital?
a)
sphere
b)
it's just too complex to think about it
c)
dumbbell
d)
I don't know this stuff.
72.

Which of the following sub-levels is correctly designated?

a)

1p5

b)

3f9

c)

2p6

d)

3d11

73.
The Heisenberg Uncertainty Principle states
a)
velocity and position cannot be determined at the same time
b)
a beam of light can interfere with the path and speed of an electron
c)
photons do not affect the position of an electron
d)
the velocity of a car cannot accurately be measured by a radar beam
74.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

75.

According to de Broglie, electrons can act like

a)

particles only.

b)

waves only.

c)

both waves and particles.

d)

spoiled brats.

76.

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

77.
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
78.

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

79.

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.

80.

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.

81.

Which of the following elements has the most "shielding" electrons?

a)

nitrogen (N)

b)

phosphorus (P)

c)

arsenic (As)

d)

bismuth (Bi)

82.

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

83.

How many shielding electrons does carbon(C) have? (hint: write its configuration first)

a)

1

b)

2

c)

3

d)

4

84.

As you go down a group, the amount of shielding....

a)

increases

b)

decreases

c)

stays the same

85.
As you go across a period, the amount of shielding...
a)
Increases
b)
decreases
c)
stays the same
86.

Which of the following elements has the most "shielding" electrons?

a)

Neon (Ne)

b)

flourine (F)

c)

oxygen (O)

d)

They have the same

87.
In the following configuration, which electrons are the shielding electrons? 1s2 2s2 2p6 3s2 3p4
a)
1s2 2s2 2p6
b)
3s2 3p4
c)
1s2 2s2
d)
2s2 2p6 3s2 3p4
88.

A photon of light with a large wavelength will have _____ energy

a)

high

b)

low

c)

the same

d)

there is no relationship between the two

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