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Periodic Trends Review 2019

Total questions: 44

Worksheet time: 4hrs 40mins

Name
Class
Date
1.

Which has the greater EN:

Cl or Al?

a)

Cl

b)

Al

2.
Which has the greater EN: 
N or C?
a)
C
b)
N
3.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
4.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
5.
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)
6.
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
7.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
8.
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
9.
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.
10.
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.
11.
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. 
12.
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
13.
Metals are good conductors of heat and electricity.
a)
true
b)
false
14.
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.
15.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
16.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

17.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
18.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
19.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
20.

When at atom gains electrons, it becomes a(n)

a)

cation

b)

anion

c)

isotope

21.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
22.

When at atom loses electrons, it becomes a(n)

a)

cation

b)

anion

c)

isotope

23.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
24.
In this picture you can see that Noble gases are not included, following the trend which one is represented?
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
25.

What is the term that describes the way in which electrons are blocked from feeling the full force of the nucleus' positive charge?

a)

multiplying

b)

Shielding

c)

growing

d)

layering

26.
Choose the element that is bigger in terms of its atomic size
a)
Al
b)
Al+2
c)
Al+3
27.
Choose the element that is bigger in terms of its atomic size
a)
O
b)
O-1
c)
O-2
28.

A measure of the size of an atom, and is generally defined as the distance from the nucleus to the outermost electron orbit

a)

chemical reactivity

b)

atomic radius

c)

energy levels

d)

orbit

29.
Which orbital block corresponds to transition metals in the periodic table?
a)
s
b)
p
c)
d
d)
f
30.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
31.

Elements in group 17 are called _______.

a)

noble gases

b)

alkali metals

c)

lanthanides

d)

halogens

32.

Metalloids that conduct electricity at high temperatures are

a)

good conductors

b)

semiconductors

c)

ductile

d)

alkaline earth metals

33.

Inner transition metals is the name for which block on the periodic table?

a)

s block

b)

p block

c)

d block

d)

f block

34.

Which is a property of nonmetals?

a)

lustrous

b)

malleable

c)

brittle

d)

good conductors

35.

Arranged the Periodic Table in order of increasing atomic mass

a)

Moseley

b)

Mendeleev

c)

Bohr

d)

Einstein

36.

Name for Groups 3-12 elements

a)

nonmetals

b)

inner transition metals

c)

transition metals

d)

metalloids

37.

The periodic table we use today is arranged in order of increasing

a)

mass

b)

number of electrons

c)

atomic radius

d)

atomic number

38.

The property of metals to be made into wire is called

a)

malleable

b)

ductile

c)

lustrous

d)

pliability

39.

An anion is ____ than its neutral form.

a)

bigger

b)

smaller

c)

the same size

d)

it depends

40.

A cation is ____ than its neutral form.

a)

bigger

b)

smaller

c)

the same size

d)

unable to tell

41.

Elements in groups 1,2 and 13-18 make up the

a)

representative elements

b)

transition elements

c)

alkali metals

42.

What group number does the electron configuration d7 end in?

a)

Group 4

b)

Group 9

c)

Group 10

43.

What electron configuration does group 2 end in?

a)

radium

b)

s2

c)

the s block

d)

the d block

44.

Which element requires the most ionization energy and what is its value?

a)

Ne, 4.1

b)

F, 4.0

c)

H, 0

d)

F, 40.0

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