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Periodic Trends

Total questions: 28

Worksheet time: 25mins

Name
Class
Date
1.

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

a)

Nitrogen (N)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

2.

Which of the following will have a lower ionization energy than Sodium (Na)?

a)

Helium (He)

b)

Lithium (Li)

c)

Potassium (K)

d)

Magnesium (Mg)

3.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
4.

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 neutrons

5.

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

a)

the atoms have more mass.

b)

The atoms have more energy levels, so more distance between the valence electrons and the nucleus, and more shielding

c)

the atoms have more protons.

d)

the atoms have less electrons.

6.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
the energy required 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
7.
Electronegativity is...
a)
how good an atom is at attracting electrons when in a compound
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. 
8.
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.
9.
The element with the largest electronegativity in the halogens is 
a)
At
b)
F
c)
Cl
d)
Br
10.
The element with the lowest electronegativity in Period 3 is 
a)
Na
b)
Cl
c)
Ar
d)
Mg
11.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
12.
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 
13.
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
14.

Which has the greater electronegativity:

Br or Ga?

a)

Br

b)

Ga

15.
Put the following elements in order of decreasing ionization energy:
O, Te, Po, S.
a)
O, S, Po, Te
b)
O, S, Te, Po
c)
O, Te, Po, S
d)
O, Po, Te, S
16.

Which is larger:

P or P3-

a)

P

b)

P3-

c)

both are same size

17.
Which is larger:
Ca  or  Ca2+
a)
Ca
b)
Ca2+
c)
both are same size
18.
Which of the following atoms would you expect  to have the largest atomic radius?
a)
Li
b)
K
c)
Ca
d)
Br
19.
Which of the following would require the most energy to remove an electron?
a)
Sodium
b)
Potassium
c)
Rubidium
d)
Cesium
20.
Which of the following Period 2 elements has the lowest ionization energy?
a)
Boron
b)
Nitrogen
c)
Beryllium
d)
Fluorine
21.
Which of the following elements has the SMALLEST atomic radius?
a)
Silicon
b)
Tin
c)
Lead
d)
Germanium
22.
Which of the following elements has the GREATEST ionization energy?
a)
Potassium
b)
Calcium
c)
Iron
d)
Selenium
23.
The Br- anion is larger than the Br atom because - 
a)
Br- has more electrons than Br, so the electron cloud is allowed to expand
b)
Br has more electrons than Br-, and more electrons repel each other
c)
Br- has more protons, so it has more attraction for its electrons
d)
Br has more protons, so it has more attraction for its electrons
24.
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, more shielding, so little energy is needed to remove it
25.
The second ionization energy for any element is always higher than the first ionization energy, because - 
a)
the number of energy levels increases with every electron removed
b)
the nuclear attraction becomes stronger with every electron removed
c)
the electron repulsion increases with every electron removed
d)
the number of neutrons increases with every electron removed
26.

Which element will have the highest 2nd ionization energy (I2)?

a)

K

b)

Ca

c)

Ga

d)

Ge

27.

Which element will have the highest 4th ionization energy (I4)?

a)

K

b)

Ca

c)

Ga

d)

Ge

28.

I1 = 1314

I2 = 3388

I3 = 5301

I4 = 7469

I5 = 10990

I6 = 13327

I7 = 71330

I8 = 84078

This element would have how many valence electrons?

a)

5

b)

6

c)

7

d)

8

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