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WorksheetsPeriodic Trends
Total questions: 45
Worksheet time: 45mins
Name
Class
Date
1.
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
2.
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
3.
The atom with the largest atomic radius in Period 4 (row 4) is -
a)
K
b)
Kr
c)
Fe
d)
Fe
4.
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, so little energy is needed to remove it
5.
The element with the smallest ionization energy in Period 6 is -
a)
Rn
b)
Cs
c)
Os
d)
Tm
6.
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.
7.
The energy required to remove electrons is the definition of:
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
8.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
9.
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)
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.
The element with the largest electronegativity in the halogens is -
a)
At
b)
F
c)
Cl
d)
Br
14.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
15.
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
16.
Which of the following is true for Calcium
a)
Metal and Low electronegativity value
b)
Metal and has 2 valence electrons
c)
Metal, Low electronegativity, has 2 valence electrons
d)
Metal and Semi conductor
17.
Which is larger:
P or P-3
P or P-3
a)
P
b)
P-3
c)
both are same size
18.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
19.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
20.
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
21.
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
22.
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.
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.
Vertical columns of elements (families) on the periodic table with similar properties
a)
groups
b)
periods
c)
quadrants
d)
rows
25.
What idea is this cartoon showing?
a)
chlorine (Cl) is more electronegative than hydrogen (H)
b)
chlorine (Cl) has more energy levels than hydrogen (H)
c)
hydrogen (H) is more electronegative than chlorine (Cl)
26.
Looking at group 2, which element has the largest atomic radius?
a)
Ba
b)
Mg
c)
Ca
d)
La
27.
Which element is the most electronegative?
a)
Hydrogen, H
b)
Aluminum, Al
c)
Oxygen, O
d)
Cesium, Cs
28.
Which of these halogens has the largest atomic radius?
a)
fluorine, F
b)
chlorine, Cl
c)
bromine, Br
d)
iodine, I
29.
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)
30.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
31.
Which of the following is a metal?
a)
Li
b)
Si
c)
S
32.
Which element has the smallest ionization energy?
a)
Na
b)
P
c)
S
33.
Which element has the largest atomic mass?
a)
K
b)
Ca
c)
Sc
34.
Which element is in the Halogen family?
a)
S
b)
Cl
c)
Ar
35.
Which element has the largest atomic radius?
a)
Ga
b)
Al
c)
Si
36.
Which element is a noble gas?
a)
Te
b)
I
c)
Xe
37.
Which element has 4 energy levels?
a)
Si
b)
Ge
c)
Sn
38.
Which element is a nonmetal?
a)
H
b)
Li
c)
Na
39.
Which element is a transition metal?
a)
Hg
b)
Si
c)
Pb
40.
Which element has an electron configuration ending in 3s23p1
a)
Na
b)
Mg
c)
Al
41.
Which element is a metalloid
a)
Pb
b)
Bi
c)
Po
42.
Which element is a gas a room temperature?
a)
B
b)
C
c)
N
43.
Which element has an electron configuration ending in 4s23d2
a)
Ca
b)
Sc
c)
Ti
44.
Which element has the smallest electronegativity?
a)
Cs
b)
Ni
c)
O
45.
The electronegativity of Cl is the highest in Period 2. 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
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