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WorksheetsPeriodic Table Trends
Total questions: 36
Worksheet time: 37mins
Name
Class
Date
1.
Which has the greatest Electronegativity:
a)
Cl
b)
Al
c)
Br
d)
He
2.
Which has the greatest 2nd ionization energy:
a)
Ca
b)
K
c)
Al
d)
Se
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.
The atom with the largest atomic radius in Group 18 is -
a)
Ar
b)
He
c)
Kr
d)
Rn
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.
The electronegativity of Cl is the highest in Period 3. 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
18.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
19.
Based on electronegativity trends in the periodic table, which of the following is the most likely value for the electronegativity of silicon?
a)
2.44
b)
1.23
c)
2.22
d)
2.03
20.
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
21.
there is an _____________ in radii of the cation compared to its atom
a)
increases
b)
decrease
c)
no change
d)
increase then decrease
22.
there is an _____________ in radii of the anion compared to its atom
a)
increase
b)
decrease
c)
no change
d)
increase then decrease
23.
the difference in the size of the anion compared to its atom is due to
a)
a loss of an energy level
b)
an increase in electron-electron repulsion
c)
a greater attraction to the nucleus
d)
less electron electron repulsion
24.
the trend of ionic radii down a group of the periodic table for the cations
a)
increases in radii
b)
decreases in radii
c)
no change in radii
d)
decreases then increases
25.
the difference in the size of the cation compared to its atom is
a)
due to the loss of an energy level
b)
all of the options
c)
feels greater attraction to the nucleus
d)
less electron electron repulsion
26.
the noble gas notation for an Al3+ ion is
a)
[He]
b)
[Ar]
c)
[Ne]
d)
[Al]3+
27.
The ions P3-, S2- and Cl- have radii of 0.212 nm, 0.184 nm and 0.181 nm respectively. This decrease in radius in going from P3- to Cl- is due to...
a)
an increase in the total number of electrons while the nuclear charge remains constant
b)
an increase in the total number of electrons and the nuclear charge
c)
an increase in the nuclear charge while the total number of electrons is the same
d)
a decrease of negative charge while the total number of electrons and the nuclear charge remains constant
28.
which element has an ion with a greater radii than its atom
a)
Mg
b)
Be
c)
K
d)
F
29.
which element has a smaller ionic radii than its atomic radii
a)
O
b)
S
c)
Se
d)
Ag
30.
As you look from left to right across a period, ionic radius
a)
increases
b)
decreases
31.
Which of these has the greatest ionic radius?
a)
potassium
b)
aluminum
c)
carbon
d)
oxygen
32.
Which of these has the greatest ionic radius?
a)
potassium
b)
aluminum
c)
carbon
d)
oxygen
33.
Which has the largest radius:
a)
Ca
b)
Ca+2
34.
Which has the largest radius:
a)
Cl
b)
Cl-
35.
Which has the largest radius
a)
F-
b)
Na+
36.
Which has the smallest radius
a)
Cl-
b)
Ar
c)
K+
d)
Br-
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