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Trends in the Periodic Table

Total questions: 50

Worksheet time: 50mins

Name
Class
Date
1.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

2.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
3.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
4.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
5.
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
6.

Which of the following elements is most likely to have similar properties to those of sodium (Na)?

a)

Magnesium (Mg)

b)

Sulfur (S)

c)

Francium (Fr)

d)

Titanium (Ti)

7.

Which element is located in period 4?

a)

Zirconium (Zr)

b)

Silicon (Si)

c)

Beryllium (Be)

d)

Iron (Fe)

8.

Which element is located in period 4 and group 5?

a)

Vanadium (V)

b)

Zirconium (Zr)

c)

Niobium (Nb)

d)

Titanium (Ti)

9.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
10.

What is the charge on a sodium ion?

a)

+2

b)

+1

c)

-2

d)

-1

11.

Elements in the same group will have

a)

the same # of orbitals

b)

all have a charge of -3

c)

the same # e in the outer shell

d)

all have a charge of +1

12.

On the periodic table, the following elements, oxygen, sulfur, selenium and tellurium are considered a

a)

group

b)

period

13.

The following elements (sodium, magnesium, aluminum, silicon, phosphorus and chlorine) are considered a

a)

group

b)

period

14.

Atomic size decreases moving right to left on the Periodic Table.

a)

true

b)

false

15.

As you move from left to right across each row of the Periodic Table, the size of an atom

a)

Decreases because additional protons and electrons are added to the same principal energy level, resulting in more forces of attraction and pulling the electrons closer to the nucleus.

b)

Increases because electrons are added to energy levels further away from the nucleus, which results in electron shielding.

c)

Decreases because electrons are more easily lost.

d)

Increases because additional neutrons added to the nucleus interfere with the forces of attraction between the protons and electrons.

16.

As you move from top to bottom down the Alkali Metal group of the Periodic Table, the size of an atom

a)

Decreases because additional protons and electrons are added to the same principal energy level, resulting in more forces of attraction and pulling the electrons closer to the nucleus.

b)

Increases because electrons are added to energy levels further away from the nucleus, which results in electron shielding.

c)

Decreases because electrons are more easily lost.

d)

Increases because additional neutrons added to the nucleus interfere with the forces of attraction between the protons and electrons.

17.

Why is the second ionization energy always greater than the first ionization energy for any element?

a)

The charge on the ion has become more positive, causing an increased attraction of the positively charged nucleus for the decreasing number of electrons.

b)

The charge on the ion has become more positive, causing a decreased attraction of the positively charged nucleus for the increasing number of electrons.

c)

The charge on the ion has become more negative, causing an increased attraction of the positively charged nucleus for the decreasing number of electrons.

d)

The charge on the ion has become more negative, causing a decreased attraction of the positively charged nucleus for the increasing number of electrons.

18.

As you move from left to right across each row of the Periodic Table, ionization energy

a)

Decreases, because additional protons are being added to the same principal energy level, leading to a weaker attraction for the electrons to the positively charged nucleus.

b)

Decreases, because additional electrons are being added to different principal energy levels, leading to a weaker attraction for the electrons to the positively charged nucleus.

c)

Increases, because additional protons are being added to the same principal energy level, leading to a greater attraction for the electrons to the positively charged nucleus.

d)

Increases, because additional electrons are being added to different principal energy levels, leading to a weaker attraction for the electrons to the positively charged nucleus.

19.

Which sequence of elements is arranged in order of decreasing atomic radii?

a)

Al, Si, P

b)

Li, Na, K

c)

Cl, Br, I

d)

N, C, B

20.

Which sequence correctly places the elements in order of increasing ionization energy?

a)

H, Li, Na, K

b)

I, Br, Cl, F

c)

O, S, Se, Te

d)

H, Be, Al, Ga

21.

Which sequence correctly places the elements in order of increasing electronegativity?

a)

Ca, Zn, Br, K, Sc

b)

Br, Zn, Sc, Ca, K

c)

Sc, K, Br, Zn, Ca

d)

K, Ca, Sc, Zn, Br

22.

Where are the metalloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

23.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
24.

Which element is most likely to have six valence electrons?

a)

Barium (Ba)

b)

Carbon (C)

c)

Oxygen (O)

d)

Americium (Am)

25.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
26.

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

27.

Which element has the highest electronegativity?

a)

Mg

b)

Al

c)

Si

d)

P

28.

Which element has the larges atomic radius?

a)

Silicon

b)

Germanium

c)

Tin

d)

Lead

29.

Which element as the smallest ionization energy?

a)

Titanium

b)

Chomium

c)

Manganese

d)

Copper

30.

Which element has the highest ionization energy?

a)

Boron

b)

Aluminum

c)

Gallium

d)

Indium

31.

Which element has the lowest electronegativity?

a)

Strontium

b)

Calcium

c)

Magnesium

d)

Beryllium

32.

What is the likelihood of a substance to undergo a chemical reaction, either by itself or with other materials, and absorb or release energy?

a)

group or family

b)

reactivity

c)

period

d)

octet rule

33.

What is a region of an atom where electrons with the same energy are found?

a)

electron

b)

orbital

c)

sublevel

d)

energy level

34.

Which element is more reactive?

a)

Li

b)

Fr

c)

Ba

35.

Which alkaline Earth metal would have the smallest radius?

a)

Be

b)

Ca

c)

Ra

36.

Which noble gas has the largest radius?

a)

Ne

b)

Kr

c)

Rn

37.
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.
38.
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
39.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
40.
a)

2

b)

3

c)

5

41.
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
42.
Which element has 2 valence electrons? 
a)
cesium (Cs) 
b)
magnesium (Mg)
c)
boron (B)
d)
argon (Ar) 
43.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
44.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

45.
How many valence electrons are in an atom of K?
a)
3
b)
8
c)
4
d)
1
46.
Which is smaller... Mg or Mg2+ ?
a)
Mg because it gains an energy level
b)
Mg due to extra electron repulsion
c)
Mg2+ because of extra electron repulsion
d)
Mg2+ because it loses an energy level
47.
Why does it take energy to remove electrons?
a)
Because it is attracted to the nucleus
b)
Because it is attracted to other electrons
c)
Because it is trapped in an orbital
d)
Because it does not want to move 
48.
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. 
49.
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
50.

An element with the lowest electronegativity would be found in of the periodic table.

a)

Group 1, Period 7

b)

Group 3, Period 4

c)

Group 5, Period 3

d)

Group 17, Period 2

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