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WorksheetsPeriodic Table Trends Periods Groups Similar Atoms
Total questions: 25
Worksheet time: 28mins
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.
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
5.
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
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.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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.
8.
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
9.
The atom with the largest atomic radius in Group 18 is -
a)
Ar
b)
He
c)
Kr
d)
Rn
10.
Metals have the largest -
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
11.
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.
12.
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
13.
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
14.
A negatively charged subatomic particle that exists in various energy levels outside the nucleus of an atom
a)
neutron
b)
electron
c)
proton
d)
subatomic particle
15.
The chart scientists use to organize and classify all the known elements
a)
elements chart
b)
the chart
c)
Periodic Table of the Elements
d)
Period table
16.
The tendency of an atom to attract electrons and acquire a negative charge
a)
electronegativity
b)
charge
c)
bonding ability
d)
electron configuration
17.
Vertical columns of elements (families) on the periodic table with similar properties
a)
groups
b)
periods
c)
quadrants
d)
rows
18.
Which region contains the halogen family of elements?
a)
right side, seventh column
b)
right side, eighteenth column
c)
left side, first column
d)
left side, second column
19.
According to ____ periodic table, the physical and chemical properties of elements are periodic functions of their atomic weights.
a)
a. Dmitri Mendeleev’s
b)
b. Henry Mosley's
c)
c. John Newland's
d)
d. Lothar Meyer’s
20.
According to ____ periodic table, the physical and chemical properties of elements are periodic functions of their atomic number.
a)
a. Dmitri Mendeleev’s
b)
b. Henry Moseley's
c)
c. John Newland's
d)
d. Lothar Meyer’s
21.
Which metalloid is in the fourth period and the same group as Carbon?
a)
a. silicon
b)
b. tin
c)
c. germanium
d)
d. boron
22.
Why is the size of a sodium ion (Na+) less than that of a sodium atom (Na)?
a)
The ion has a full energy level because it gained one electron.
b)
The ion has a full energy level because it lost one electron.
c)
The ion make the octet, but the atom does not.
d)
Answers b and c are correct.
23.
An element has similar chemical properties as oxygen and selenium. It has an atomic number greater than krypton but less than iodine. Use the periodic table to identify the element.
a)
selenium
b)
polonium
c)
sulfur
d)
tellurium
24.
Why do elements in the same group have similar properties?
a)
They have the same number of energy levels.
b)
They have the same number of protons.
c)
They have the same number of electrons.
d)
They have the same number of valence electrons.
25.
When an atom loses electrons, its radius gets _____________.
a)
smaller
b)
larger
c)
remain the same
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