WorksheetsPeriodic Table & Trends
Total questions: 20
Worksheet time: 20mins
Name
Class
Date
1.
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)
2.
Which element is located in group 3?
a)
Yttrium (Y)
b)
Carbon (C)
c)
Sodium (Na)
d)
Lithium (Li)
3.
Which element is most likely to have three electron energy levels?
a)
Argon (Ar)
b)
Lithium (Li)
c)
Boron (B)
d)
Europium (Eu)
4.
Which element is located in period 4 and group 5?
a)
Vanadium (V)
b)
Zirconium (Zr)
c)
Niobium (Nb)
d)
Titanium (Ti)
5.
Which element is most likely to have six electrons in its 4th energy level?
a)
Oxygen (O)
b)
Selenium (Se)
c)
Krypton (Kr)
d)
Potassium (K)
6.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium
c)
francium
d)
cesium
7.
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
8.
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.
9.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
10.
Order the following in increasing atomic radii:
Ra, Be, Ca, Rb, H
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
11.
The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?
a)
The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.
b)
The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.
c)
The ionization energy increases gradually as you move right across a period because you are adding more protons.
d)
The ionization energy increases when the valence electrons are more attracted to the nucleus.
12.
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
13.
Which of the following is true about a sulfur atom and a chlorine atom?
a)
Sulfur is larger and has higher ionization energy.
b)
Sulfur is larger and has lower ionization energy.
c)
Sulfur is smaller and has higher ionization energy.
d)
Sulfur is smaller and has lower ionization energy.
14.
Which element has the greater ionization energy?
a)
Strontium
b)
Boron
15.
Put the following in order of increasing ionization energy:Sodium, Oxygen, Boron
a)
Sodium, Boron, Oxygen
b)
Oxygen, Boron, Sodium
c)
Sodium, Oxygen, Boron
d)
Oxygen, Sodium, Boron
16.
Choose the set that goes from lowest to highest electronegativity?
a)
Cu, Mg, Sr, Ca
b)
F, Cl, Br, Si
c)
Cs, Rb, Ca, Mg
d)
Zn, Cd, Ag, Cu
17.
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.
18.
Which of the following generally applies to the noble gases?
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity
19.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
20.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
100 %
