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Chapter 5 review- periodic trends

Total questions: 54

Worksheet time: 42mins

Name
Class
Date
1.
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
2.
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 and electrons

d)

the atoms have fewer protons and electrons

3.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
4.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
5.
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
6.
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)
7.
Which of the following will have a higher ionization energy than arsenic (As)?
a)
Gallium (Ga)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
8.
Electronegativity is...
a)

how well an atom is at attracting electrons while bonded

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. 
9.
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.
10.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
11.
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
12.

The electronegativity of Cl is the highest in Period 3.  Why?

a)
Cl is the largest and has the greatest effective nuclear charge
b)
Cl is the smallest and has the lowest effective nuclear charge
c)
Cl is the largest and has the lowest effective nuclear charge
d)
Cl is the smallest and has the greatest effective nuclear charge
13.
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
14.
What term is used to describe "The energy required to remove an electron from gaseous atoms"
a)
excitation energy
b)
ionization energy
c)
polarization energy
d)
electrolytic energy 
15.

Which has the greater electronegativity?

a)
Cl
b)
Al
c)

P

d)

Mg

16.

Which has the greater Electronegativity?

a)
C
b)
N
c)

B

d)

Li

17.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
18.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
19.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
20.
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.
21.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
22.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Mg

d)

Al

23.
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
24.

The larger the atom the

a)

smaller the ionization energy

b)

larger the ionization energy

25.

The closer an atom is to F what happens to its electronegativity?

a)

It gets bigger

b)

It gets smaller

26.

Put these is order from largest to smallest.


V, K, Ni

a)

K > V > Ni

b)

Ni > V > K

c)

V > Ni > K

d)

K > Ni > V

27.

Put these is order from largest to smallest.

As, Sb, N

a)

Sb > As > N

b)

N > Sb > As

c)

N > As > Sb

28.

Which has the larger first ionization energy?

a)

Ca

b)

Se

c)

P

d)

O

29.
Name group 1 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
noble gases
d)
halogens
30.
Name group 2 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
31.
Name group 18 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
noble gases
32.
Name groups 3 - 12 on the periodic table.
a)
noble gases
b)
halogens
c)
metalloids
d)
transition metals
33.
Name group 17 on the periodic table.
a)
transition metals
b)
metalloids
c)
halogens
d)
alkali metals
34.
Which group has the most reactive nonmetals?
a)
alkali metals
b)
noble gases
c)
metalloids
d)
halogens
35.
Name the group that contains inert (nonreactive) elements.
a)
noble gases
b)
halogens
c)
alkali metals
d)
alkaline earth metals
36.
What do the numbers down the side tell us about the atoms in each row?
a)
number of protons
b)
number of electrons
c)
number of energy levels
d)
absolutely nothing
37.

F Block atoms are called

a)

inner transition metals

b)

outer transition metals

c)

transition metals

d)

non-metals

38.

F block atoms can be paramagnetic (partially magnetic)

a)

true

b)

false

39.

These have some properties of metals and non-metals. They are semiconductors.

a)

metalloids

b)

metals

c)

non-metals

d)

gases

40.

Where are the group numbers?

a)

At the top of each column on the periodic table

b)

On the right side of each row on the periodic table

c)

Under the element name on the periodic table

41.

Period numbers tell..

a)

how many energy levels the atom has.

b)

how many electrons an atoms has

c)

how many neutrons an atom has

d)

which group an atom is in

42.

Match the following

a)

The most electronegative element

1.

F

b)

The smallest atom

2.

He

c)

The second most electronegative element

3.

O

d)

The least electronegative element

4.

Fr

e)

A non-metal that is a liquid at room temperature

5.

Br

43.
Question Image

Match the following

a)

Usually has a +1 charge

1.

Na

b)

Usually has a +2 charge

2.

Ba

c)

Usually has a -1 charge

3.

Cl

d)

Usually has a -2 charge

4.

O

e)

Usually has a +3 charge

5.

Al

44.

This non-metal is usually solid at room temperature and looks like little gray pieces or balls

a)

Fluorine

b)

Iodine

c)

Arsenic

d)

Chlorine

45.

Gets credit for the modern periodic table

a)

Dalton

b)

Rutherford

c)

Mendeleev

d)

Bohr

46.

the amount of energy required to add an electron to a neutral atom to form an anion

a)

electron affinity

b)

electronegativity

c)

ionization energy

47.

A cation has what charge?

a)

negative

b)

positive

48.
a)

This is the Bohr model of Cs

b)

This is the quantum model of Cs

c)

This is the nuclear model of Cs

49.
Question Image

Match the following

a)

removing an electron forms a(an)

1.

cation

b)

adding an electron forms a(an)

2.

anion

c)

which family has 5 valence electrons

3.

Nitrogen family

d)

which family has 4 valence electrons

4.

carbon family

e)

which family has 3 valence electrons

5.

boron family

50.

This reacts like group 1 (1 valence electron) and reacts like group 17 (only needs 1 electron to complete its outer shell)

a)

He

b)

H

c)

Li

d)

F

51.

How is electronegativity determined?

a)

no clue

b)

experimentally

c)

we guess

d)

by thinking about the atoms

52.

Why are anions larger than their parent atoms?

a)

Extra electrons act like shields and extra electrons are repelled by the other electrons

b)

because you add an energy level to the atom

c)

because atoms want more electrons

d)

because atoms want fewer electrons

53.

Why are cations smaller than the parent atoms?

a)

because you add another electron and lower the energy levels

b)

because you remove an electron and lower the number of energy levels

c)

because parent atoms are always bigger than cations and anions

d)

because you add a proton and pull in the electrons more

54.
Question Image

Match the following

a)

group 1, period 4

1.

K

b)

group 8, period 5

2.

Ru

c)

group 8A, period 3

3.

Ar

d)

group 3A, period 4

4.

Ga

e)

group 3, period 4

5.

Sc

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