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Periodic Table and Trends

Total questions: 100

Worksheet time: 3hrs 20mins

Name
Class
Date
1.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
2.
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. 
3.
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
4.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
5.

As you move from left to right on the periodic table, the number of valence electrons.......

a)

Increases

b)

Decreases

c)

Remains the same

6.

As you move down a group on the periodic table, the number of valence electrons....

a)

Increases

b)

Decreases

c)

Remains the same

7.

Which of the following would be most similar to Phosphorus? (select all that apply)

a)

Nitrogen

b)

Sulfur

c)

Silicon

d)

Germanium

e)

Antimony

8.

The common charge on an atom in group 17 would be....

a)

+1

b)

+7

c)

-7

d)

-1

e)

17

9.

Which of the following reasons explains why there is a decimal for most atomic masses?

a)

The mass of one atom can have a fraction.

b)

Since electrons are very small mass they only add a little bit, usually only a decimals worth.

c)

It is the average mass of all the potential isotopes of an atom.

d)

Neutrons have a mass of 1.1 meaning that fractions are common.

10.

Which of the following is true of atomic radius?

a)

The radius is mainly due to how large an atom's nucleus is.

b)

The radius is mainly due to the size of the electron cloud.

c)

The atomic radius is a way we measure the mass of an atom.

d)

Neutrons account for the majority of an atom's radius.

11.

Which of the following is the term for a substance in which all the atoms have the same number of protons

a)

a compound

b)

An element

c)

a molecule

d)

a solid

e)

a gas

12.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

13.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
14.
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
15.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
16.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
17.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
18.

Which of the following are physical properties of metal?

a)

Luster

b)

Conductivity

c)

Malleability

d)

Ductility

19.

True or False: The reactivity of metals tends to decrease as you move from left to right across the periodic table.

a)

True

b)

False

20.

Name this group: These metals are the most reactive.

a)
b)
c)
d)
21.

Name this group: These metals are the second most reactive.

a)
b)
c)
d)
22.

Name this group: These metals are the second most reactive.

a)
b)
c)
d)
23.

Name this group: These metals contain familiar metals such as gold, iron, and copper.

a)
b)
c)
d)
24.

Name this group: These metals, located near the nonmetals, are never found uncombined in nature.

a)
b)
c)
d)
25.

Find these groups: Locate Lanthanides and Actinides.

a)
b)
c)
d)
26.

Which of the following could be properties of nonmetals?

a)

Poor electrical conductivity

b)

Poor thermal conductivity

c)

Dullness

d)

Brittleness

27.

I am a metal


I am in group 2


I am in period 6


I am…

a)

Mo

b)

Re

c)

S

d)

Ba

28.

I am a nonmetal


I am in period 2


I am in group 16/6A

a)

Ba

b)

Si

c)

Ba

d)

O

29.

Find an element with similar chemical properties to Barium (Ba).

a)

Ca an Ra, because they are in the same group and have similar chemical properties.

b)

Cs and La, b/c they are in the same period number.

c)

Ca and Y, b/c they are 90 degree angle and have similiar properties.

30.

The energy it takes to remove one electron from an atom

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

31.

The distance between nucleus and outermost shell occupied electron

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

32.

The tendency of an atom to attract a shared pair of electrons

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

33.

The amount of energy released when an electron is added to a neutral atom to form a negative ion

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

34.

The degree of oxidation (loss of electrons) of an atom in a chemical compound

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

35.

Atomic radii trends is . . . .

a)

generally decrease along each period of the table, from the alkali metals to the noble gases; and increase down each group.

b)

generally increase along each period of the table, from the alkali metals to the noble gases; and increase down each group.

c)

generally increase along each period of the table, from the alkali metals to the noble gases; and decrease down each group.

d)

generally decrease along each period of the table, from the alkali metals to the noble gases; and decrease down each group.

36.

Ionization energy trends is . . . .

a)

becomes greater up and to the right of the periodic table.

b)

becomes greater down and to the right of the periodic table.

c)

becomes greater up and to the left of the periodic table.

d)

becomes greater down and to the left of the periodic table.

37.

Electronegativity trends is . . . .

a)

increases on passing from left to right along a period, and decreases on descending a group.

b)

increases on passing from left to right along a period, and increases on descending a group.

c)

decreases on passing from left to right along a period, and decreases on descending a group.

d)

decreases on passing from left to right along a period, and increases on descending a group.

38.

Electron affinity trends is . . . .

a)

generally increases across a period, and a trend of decreasing electron affinity going down groups would be expected.

b)

generally decreases across a period, and a trend of decreasing electron affinity going down groups would be expected.

c)

generally increases across a period, and a trend of increasing electron affinity going down groups would be expected.

d)

generally decreases across a period, and a trend of increasing electron affinity going down groups would be expected.

39.

Metallic character trends is . . . .

a)

decrease going across a period and tends to increase going down a group.

b)

increase going across a period and tends to increase going down a group.

c)

decrease going across a period and tends to decrease going down a group.

d)

increase going across a period and tends to decrease going down a group.

40.

Which element has smaller atomic radii?

a)

Beryllium is smaller than Fluorine

b)

Sulphur is smaller than Oxygen

c)

Litihium is smaller than Sodium

d)

Potassium is smaller than Bromine

41.

Which element has higher ionization energy?

a)

Chlorine is higher than Sodium

b)

Phosphorus is higher than Nitrogen

c)

Silicon is higher than Carbon

d)

Magnesium is higher than Aluminium

42.

Which element has lower ionization energy?

a)

Chlorine is lower than Sodium

b)

Phosphorus is lower than Nitrogen

c)

Carbon is lower than Silicon

d)

Aluminium is lower than Magnesium

43.

Which element has higher electronegativity?

a)

Fluorine is higher than Oxygen

b)

Potassium is higher than Sodium

c)

Aluminium is higher than Boron

d)

Phosphorus is higher than Chlorine

44.

Which element has lower electronegativity?

a)

Fluorine is lower than Oxygen

b)

Potassium is lower than Sodium

c)

Boron is lower than Aluminium

d)

Chlorine is lower than Phosphorus

45.

Which element has higher electron affinity?

a)

Bromine is higher than Calsium

b)

Chlorine is higher than Fluorine

c)

Magnesium is higher than Beryllium

d)

Sodium is higher than Aluminium

46.

Which element has bigger atomic radii?

a)

Beryllium is bigger than Fluorine

b)

Oxygen is bigger than Sulphur

c)

Litihium is bigger than Sodium

d)

Phosphorus is bigger than Bromine

47.

Which element has lower electron affinity?

a)

Bromine is lower than Calsium

b)

Chlorine is lower than Fluorine

c)

Berylliumis lower than Magnesium

d)

Aluminium is lower than Sodium

48.

Which element is more metallic?

a)

Sodium is more metallic than Aluminium

b)

Fluorine is more metallic than Beryllium

c)

Potassium is more metallic than Lithium

d)

Chlorine is more metallic than Silicon

49.

Which element is less metallic?

a)

Sodium is less metallic than Aluminium

b)

Beryllium is less metallic than Fluorine

c)

Lithium is less metallic than Potassium

d)

Chlorine is less metallic than Silicon

50.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

51.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
52.
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
53.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
54.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
55.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
56.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
57.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
58.
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
59.
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)
60.
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. 
61.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
62.
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
63.
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.
64.
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
65.
How many valence electrons are in an atom of K?
a)
3
b)
8
c)
4
d)
1
66.
How many valence electrons are in an atom of Ar?
a)
2
b)
8
c)
4
d)
1
67.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
68.
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)
69.
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. 
70.
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
71.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
72.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
73.

Put these in order of INCREASING electronegativity (low to high) : O, Ra, Fe

(a)  

74.

Put these in order of INCREASING First Ionization Energy (low to high) : Ga, Ne, Rf

(a)  

75.

Which of the following describe(s) the atomic radius trend? (You may choose more than one answer)

a)

Increases Left to Right across the periodic table

b)

Increases Right to Left across the periodic table

c)

Increases Top to Bottom on the periodic table

d)

Increases Bottom to Top on the periodic table

76.

Which of the following describe(s) the Metal Reactivity trend? (You may choose more than one answer)

a)

Increases Left to Right across the periodic table

b)

Increases Right to Left across the periodic table

c)

Increases Top to Bottom on the periodic table

d)

Increases Bottom to Top on the periodic table

77.

Which of the following describe(s) the Electronegativity trend? (You may choose more than one answer)

a)

Increases Left to Right across the periodic table

b)

Increases Right to Left across the periodic table

c)

Increases Top to Bottom on the periodic table

d)

Increases Bottom to Top on the periodic table

78.

Which of the following describe(s) the First Ionization Energy trend? (You may choose more than one answer)

a)

Increases Left to Right across the periodic table

b)

Increases Right to Left across the periodic table

c)

Increases Top to Bottom on the periodic table

d)

Increases Bottom to Top on the periodic table

79.

What is the trend for metal reactivity going down a group on the periodic table?

a)

Metal reactivity decreases going down a group

b)

Metal reactivity increases going down a group

c)

Metal reactivity stays the same going down a group

d)

There is no effect on metal reactivity going down a group

80.

What happens to metal reactivity as you go across the periodic table?

a)

Decreases

b)

Increases

c)

Stays the Same

d)

Has no effect

81.

When nonmetals react, they gain electrons. 

a)

True

b)

False

82.

What is the trend for nonmetals reactivity as they go down a group on the periodic table? 

a)

Nonmetals reactivity stays the same as they go down a group on the periodic table

b)

Nonmetals reactivity increases as they go down a group on the periodic table

c)

Nonmetals reactivity decreases as they go down a group on the periodic table

d)

There is no effect on the reactivity of nonmetals as they go down a group on the periodic table

83.

According to the Octet Rule, atoms want ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

84.

Which of the following elements GAINS 1 electron in order to attain an octet?

a)

Na

b)

Ca

c)

He

d)

Cl

85.

How many valence electrons does Be have?

a)

1

b)

2

c)

4

d)

6

86.

When atoms LOSE electrons, they get a...

a)

Positive (+) charge

b)

Negative (-) charge

c)

No charge (zero)

87.

Boron (B) needs to lose 3 electrons to satisfy the Octet Rule. What is the resulting charge of the B ion?

a)

+ 3

b)

- 3

c)

+ 6

d)

Zero

88.

When atoms GAIN electrons, they get a...

a)

Positive (+) charge

b)

Negative (-) charge

c)

No charge (zero)

89.

When fluorine gains 1 electron to satisfy the Octet Rule, what is the resulting charge of the ion?

a)

+ 1

b)

- 1

c)

Zero

90.

What does Oxygen have to do to satisfy the Octet Rule? What would its charge be after? (TAKE YOUR TIME!)

a)

Lose 6 electrons, + 6

b)

Gain 8 electrons, - 8

c)

Lose 2 electrons, + 2

d)

Gain 2 electrons, - 2

91.

Which group already satisfies the Octet Rule and therefore does not bond with other atoms?

a)

Group 1 (H at top)

b)

Group 2 (Be at top)

c)

Group 13 (B at top)

d)

Group 18 (He at top)

92.

Which 2 atoms are EXCEPTIONS to the Octet Rule and only need 2 valence electrons?

a)

H, Na

b)

H, He

c)

He, Ne

d)

There are no exceptions to the Octet Rule

93.

Which of the following will form a cation?

a)

Aluminum

b)

Sulfur

c)

Iodine

d)

Nitrogen

94.

Which of the following will form an anion?

a)

Tin

b)

Lead

c)

Chlorine

d)

Zinc

95.

Which of the following will form a cation?

a)

Barium

b)

Phosphorous

c)

Tellurium

d)

Selenium

96.

Cations

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

97.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

98.

A Beryllium atom that has lost 2 electrons would look like

a)

Be2+

b)

B2-

c)

B2+

d)

Be2-

99.

The cation Rb+ has

a)

Had nothing happen to it

b)

Gained 1 electron

c)

Lost 1 electron

d)

Become negative

100.

Describe the anion S2-

a)

Silicon that gained 2 electrons

b)

Sulfide that gained 2 electrons

c)

Sulfur that gained 2 electrons

d)

Strontium that gained 2 electrons

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