Font size
WorksheetsPeriodic Table Test Review
Total questions: 79
Worksheet time: 2hrs 36mins
The Periodic Table is organized by increasing
charges
atomic number
mass number
electronegativity
The elements in the middle of the table are called the _____________ metals because their properties change from metallic to nonmetallic.
positive
negative
magnetic
transition
The _________________ are a small group of elements that have both metallic and nonmetallic properties.
Oxygen Group
Nitrogen Group
Metalloids
Halogens
The vertical columns on the periodic are called _______________.
Rows
Periods
Groups
Valence
The horizontal rows of the Periodic Table are called ______________.
Periods
Groups
Families
Halogens
The _______________electrons are the electrons on the outer most energy level of the atom.
valence
core
excited
ground state
Elements of the same ______________ have the same number of valence electrons, which determines the elements chemical properties.
Period
Row
Group
This element does not match the properties of any other group so it stands alone. It is placed above Group 1 but it is not part of that group. It is very reactive, colorless, odorless, and a gas at room temperature.
Hydrogen
Helium
Nitrogen
Oxygen
Group 1: These metals are extremely reactive. They all have one valence electron. They are shiny and silver in color. They are soft and can be cut with a knife.
Transition Metals
Alkali Metals
Alkaline Metals
Lanthanides
Group 2: Slightly less reactive because they have 2 valence electrons. They are silver colored and more dense that Group 1 metals.
Transition Metals
Alkali Metals
Alkaline-earth Metals
Actinides
Groups 3-12: These metals have a moderate range of reactivity and a wide range of properties. They are shiny and good conductors of heat and electricity. They have higher densities and melting points than Groups 1 and 2. These have 1 or 2 valence electrons.
Transition Metals
Alkali Metals
Alkaline-earth Metals
Lanthanides
Elements with atomic numbers 57-70 and 89-102: These metals were taken out and placed at the bottom of the table so the table wouldn't be so wide. Some are shiny and reactive. Others are radioactive and unstable. Elements 95-103 do not exist in nature but have been manufactured in the lab.
Alkali Metals
Alkaline-earth Metals
Lanthanides and Actinides
Boron Group
Group 13: Contains on metalloid and 4 metals. They are reactive. All have 3 valence electrons (Group # minus 10).
Boron Group
Nitrogen Group
Oxygen Group
Carbon Group
Group 14: Contains one nonmetal, two metalloids, and two metals. These all have 4 valence electrons (Group # minus 10) and have varied reactivity.
Boron Group
Carbon Group
Nitrogen Group
Oxygen Group
Group 15: Contains two nonmetals, two metalloids, and one metal. They have varied reactivity. These elements have 5 valence electrons (Group # minus 10).
Boron Group
Carbon Group
Nitrogen Group
Oxygen Group
Group 16: Contains three nonmetals, one metalloid, and one metal. They are a reactive group. These elements all have 6 valence electrons (Group # minus 10).
Boron Group
Carbon Group
Nitrogen Group
Oxygen Group
Group 17: All nonmetals. Very reactive. Poor conductors of heat and electricity. Tend to form salts with metals. Example NaCl: sodium chloride which is known as table salt. These elemtns have 7 valence electrons (Group # minus 10).
Boron Group
Oxygen Group
Nitrogen Group
Halogens
Group 18: Unreactive nonmetals. All are colorless, odorless gases at room temperature. These elements have a full outer energy level, usually 8 valence electrons, except for Helium which only has 2 valence electrons.
Nitrogen Group
Oxygen Group
Noble Gases
Halogens
The elements on the right side of the Periodic Table are classified as ________________.
Metals
Nonmetals
The elements on the left side of the periodic table are classified as ________________.
metals
nonmetals
Which is NOT a property of metals?
brittleness
conductivity
ductility
luster
What are two properties that make a metal a good choice to use as wire in electronics?
conductivity, malleability
ductility, conductivity
luster, malleability
malleability, high density
Iodine is a nonmetal. What is one property of iodine?
conductivity
dull appearance
malleability
ductility
How many valence electrons in this atom?
12
7
8
14
What is the charge of an element in Group 1?
0
+1
-1
+2
What is the charge of an element in Group 2?
+2
0
+1
-2
What is the charge of an element in Group 13?
+1
-3
+3
+2
What is the charge of an element in Group 14?
+2
-4
+4
+6
What is the charge of an element in Group 15?
+2
+3
-3
-1
What is the charge of an element in Group 16?
-2
0
+2
-1
What is the charge of an element in Group 17?
-1
+2
+1
0
What is a positive ion called?
anion
cation
isotope
covalent
The ability to attract an electron in a chemical bond
electronegativity
electron affinity
metallic character
ionization energy
The element with the highest electronegativity is -
At
F
Cl
Br
(select 2) Atomic Radius increases as you move
Down a Group
Up a Group
Left to Right across a Period
Right to Left across a Period
(select 2) Electronegativity energy increases as you move
Down a Group
Up a Group
Left to Right across a Period
Right to Left across a Period
N or C?
Which of the following halogens has the greatest electronegativity?
Chlorine (Cl)
Bromine (Br)
Iodine (I)
Astatine (At)
Which atom has the lowest electronegativity?
Lithium (Li)
Oxygen (O)
Neon (Ne)
Which of the following atoms would have the highest ionization energy?
Francium (Fr)
Zinc (Zn)
Tin (Sn)
Chlorine (Cl)
Which element has the smallest atomic radius?
Lithium (Li)
Francium (Fr)
Fluorine (F)
Radon (Rn)
Most of the elements on the periodic table are nonmetals.
True
False
What property is being measured in this diagram?
Density
Ionization Energy
Atomic Radius
Atomic Mass
What is the molar mass of magnesium?
54.94 g/mol
1 g/mol
40.08 g/mol
24.31 g/mol
What is the molar mass of sodium chloride, NaCl?
58.44 g/mol
1 g/mol
75.53 g/mol
22.99 g/mol
What is the molar mass of Cl2?
17 g/mol
35.5 g/mo;
71.0 g/mol
89 g/mol
Calculate the molar mass of KOH.
28 g/mol
56 g/mol
84 g/mol
112 g/mol
Calculate the molar mass of CO2.
14 g/mol
28 g/mol
36 g/mol
44 g/mol
Calculate the molar mass for Al(OH)3
78.0 g/mol
72 g/mol
28 g/mol
25 g/mol
The "Law of Octaves" was the brainchild of
Glenn Seaborg
Lothar Meyer
Johann Dobereiner
John Newlands
The idea of "triads" of elements with similar properties was due to
John Newlands
Johann Dobereiner
Dmitri Mendeleev
Henry Moseley
The scientist ____ is credited with the idea of arranging the elements in the periodic table according to their physical and chemical properties.
Mendeleev
Dobereiner
Newlands
Dalton
Mendeleev predicted that the empty spaces in his periodic table represented ____.
isotopes
radioactive elements
permanent gaps
undiscovered elements
