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Periodic Table Trends

Total questions: 70

Worksheet time: 5hrs 33mins

Name
Class
Date
1.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
2.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
3.
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)
4.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
5.
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
6.
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 
7.

Vertical columns of elements (these are also known as a "family") - they also have the same number of valence electrons and are known as ________________.

a)

groups

b)

periods

c)

quadrants

d)

rows

8.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
9.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
10.

Most noble gases have _______ valence electrons.

a)

1

b)

2

c)

7

d)

8

11.
In what section would Noble Gases be found?
a)
white
b)
yellow
c)
blue
d)
red
12.

Group 3 elements have ____ electrons in their outermost shell.

a)

1

b)

2

c)

3

d)

4

13.

What is the oxidation number of Magnesium (Mg)?

a)

+2

b)

-2

c)

+4

d)

-4

14.
What is the oxidation number for Flourine (F)?
a)
+1 
b)
-1
c)
17
d)
7
15.

Which two elements on the periodic table are in the same period?

a)

Sn and Rb

b)

K and Ba

c)

F and Cl

d)

Se and Te

16.

What is the charge for an ion in group 3?

a)

+3

b)

-7

c)

-3

d)

+4

17.

The horizontal rows on the periodic table, which indicate the number of energy levels/orbitals that an atom has, are called ___________.

a)

Periods

b)

Element

c)

Atomic Number

d)

Group

18.

Which element would have the same number of energy levels or orbitals as Zinc?

a)

Cadmium

b)

Krypton

c)

Silver

d)

Tin

19.

Rank the following from lowest ioniziation energy to highest ionization energy: C, P, S, As

a)

C, P, S, As

b)

As, C, P, S

c)

P, S, As, C

d)

C, As, P, S

20.

Rank the following in order of increasing reactivity: Ge, K, Br, Ca (lowest to highest reactivity)

a)

Ge, K, Br, Ca

b)

K, Br, Ge, Ca

c)

Br, Ge, Ca, K

d)

Br, Ca, Ge, K

21.

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

a)

Increases

b)

Decreases

c)

Remains the same

22.

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

a)

Increases

b)

Decreases

c)

Remains the same

23.

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

24.

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.

25.
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
26.
The ionization potential of an element is the amount of energy required to remove an electron from an isolated atom or molecule. According to the periodic table, which of the following indicates the correct decreasing order of ionization energy?
a)
Li > Na > K > Cs
b)
Na > K > Li > Cs
c)
Li > K > Na > Cs 
d)
Cs > K > Na > Li 
27.
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
28.
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
29.
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
30.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
31.
Which element has 2 valence electrons? 
a)
cesium (Cs) 
b)
magnesium (Mg)
c)
boron (B)
d)
argon (Ar) 
32.
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)
33.
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. 
34.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
35.
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
36.

The metals are located

a)

to the left of the stair step.

b)

to the right of the stair step.

c)

on and around the stair step.

37.

The metalloids are located

a)

to the left of the stair step.

b)

to the right of the stair step.

c)

on and around the stair step.

38.

Metals are MOSTLY _____ at room temperature.

a)

solid

b)

liquid

c)

gas

39.

Nonmetals are MOSTLY _____ at room temperature.

a)

solid

b)

liquid

c)

gas

40.

Nitrogen is a

a)

metal.

b)

nonmetal.

c)

metalloid.

41.
As we move across a period, the ionization energy (energy needed to lose an electron and make an ion)
a)
increases
b)
decrease
c)
increases then decrease
d)
does not change
42.
As we move across a period, the metallic properties
a)
increases
b)
decrease
c)
increases then decrease
d)
does not change
43.
As we move down a group, the ionization energy (energy needed to lose an electron and make an ion)
a)
increases
b)
decrease
c)
increases then decrease
d)
does not change
44.
As we move across a period, the atomic radius (atom size)
a)
increases
b)
decrease
c)
increases then decrease
d)
does not change
45.
As we move down a group, the atomic radius (atom size)
a)
increases
b)
decrease
c)
increases then decrease
d)
does not change
46.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
47.
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
48.
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
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.
Rutherford's experiment showed that most of an atom is made up of _____.
a)
a nucleus
b)
an electron cloud
c)
empty space
d)
alpha particles
51.
Why do noble gases have the highest first ionization energies?
a)
The principal quantum number increases left to right across the periodic table.
b)
The effective nuclear charge is low.
c)
The electron affinity is zero.
d)
An electron is harder to remove from a noble gas due to it being tightly bound by the inner nucleus.
52.
Despite the fact that lithium is prescribed in the form of lithium salt for the treatment of bipolar disorder, the element lithium is unsuitable for human consumption due to its violent reaction with water. 
What could be a possible reason for its reaction with water?
a)
Low atomic mass.
b)
Low ionization energy.
c)
Oxidation state of +1.
d)
High electron affinity.
53.
Arrange the following isoelectronic ions in INCREASING order of atomic radius.
a)
S2- < Cl- < K+ < Ca2+ < Sc3+
b)
K+ < Ca2+ < Sc3+ < Cl- < S2-
c)
Sc3+ < Ca2+ < K+ < Cl- < S2-
d)
Cl- < S2- < K+ < Ca2+ < Sc3+
54.
A rule that states that repeating chemical and physical properties of elements change periodically with the atomic number of the elements is the _________.
a)
periodic law
b)
alkaline-earth metals
c)
actinide
d)
group rule
55.
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
56.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
57.
All of the actinides are ___________.
a)
stable
b)
radioactive
c)
shiny
d)
named after scientists
58.

Which scientist developed the first published periodic table where elements were placed in order of increasing atomic mass?

a)

Henry Moseley

b)

Johann Dobereiner

c)

John Dalton

d)

Dmitri Mendeleev

59.

Which periodic trend has to do with the width of a given atom?

a)

Ionic Radius

b)

Atomic Radius

c)

Electronegativity

d)

Reactivity

60.

Elements in the same group have similar _______.

a)

Atomic Mass

b)

Symbol

c)

Chemical Properties

d)

Atomic Number

61.

The element with the highest electronegativity in the halogen group?

a)

At

b)

F

c)

Cl

d)

Br

62.

The minimum energy required to remove an electron from the ground state of an atom

a)

electron configuration

b)

energy levels

c)

ionization energy

d)

ionic bond

63.

Which of the following is in the correct order of size?

a)

Anion > Atom > Cation

b)

Atom > Cation > Anion

c)

Cation > Atom > Anion

d)

Anion > Cation > Atom

64.
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
65.

Which group has "zero" electronegativity?

a)

Transition Metals

b)

Alkali Metals

c)

Noble Gases

d)

Halogens

66.

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

67.
The minimum energy required to remove an electron from the ground state of an atom
a)
electron configuration
b)
energy levels
c)
ionization energy
d)
ionic bond
68.
The energies of electrons as they orbit the nucleus of an atom
a)
energy levels
b)
orbits
c)
shells
d)
electron area
69.
Vertical columns of elements (families) on the periodic table with similar valence electron configurations and similar properties
a)
groups
b)
periods
c)
quadrants
d)
rows
70.
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

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