WorksheetsPeriodic Table/Trends and Ionic Bonds Study Guide (Grade 12)
Total questions: 62
Worksheet time: 31mins
Who wrote the first recognizable modern periodic table?
Dmitri Mendeleev
Henry Moseley
Antoine Lavoisier
John Newlands
How is the periodic table arranged?
By increasing atomic number
By increasing atomic mass
Alphabetically by element name
By melting point
What are the columns that go up and down called?
Groups
Periods
Series
Blocks
What are the across rows called?
Periods
Groups
Families
Levels
Elements in the same group have the same what?
Number of valence electrons
Atomic number
Mass number
Number of protons
Elements in the same period have the same what?
Number of occupied energy levels (electron shells)
Number of valence electrons
Atomic number
Neutron count
What is the name of group 1 in the periodic table?
Alkali metals
Alkaline earth metals
Transition metals
Halogens
What is the name of group 2 in the periodic table?
Alkaline earth metals
Alkali metals
Transition metals
Noble gases
What are groups 3–12 called?
Transition metals
Inner transition metals
Metalloids
Lanthanides
What is the name of group 17?
Halogens
Noble gases
Alkali metals
Alkaline earth metals
What is the name of group 18?
Noble gases
Halogens
Transition metals
Metalloids
Which two groups are the most reactive?
Group 1 (alkali metals)
Group 2 (alkaline earth metals)
Group 17 (halogens)
Group 18 (noble gases)
Which group is the most stable, and why?
Group 18 (noble gases) because they have full valence shells
Group 1 (alkali metals) because they have low density
Group 2 (alkaline earth metals) because they are metals
Group 17 (halogens) because they are highly electronegative
What are atomic radii?
The distance from the nucleus to the outermost electron level (a measure of atomic size)
The number of neutrons in an atom
The energy required to remove an electron
The charge on the nucleus
What is the trend for atomic radii?
Increase down a group and decrease from left to right across a period
Decrease down a group and increase from left to right across a period
Stay constant across periods and increase down groups
Increase toward the center of the table
Explain why the size of an atom decreases as you move from left to right.
Effective nuclear charge increases across a period, pulling electrons closer while shielding remains similar
Shielding increases dramatically across a period, pushing electrons outward
Electron shells are added across a period, increasing atomic size
Protons are lost across a period, reducing nuclear pull
Which atom would have the larger atomic radius: Ba atom or Ra atom?
Ba atom
Ra atom
Which atom would have the larger atomic radius: B atom or In atom?
B atom
In atom
Which atom would have the larger atomic radius: Mn atom or Re atom?
Mn atom
Re atom
Which atom would have the larger atomic radius: As atom or Cl atom?
As atom
Cl atom
What is ionization energy?
The energy required to remove an electron from a gaseous atom
The energy released when an atom gains an electron
The tendency of an atom to attract electrons in a bond
The energy stored in the nucleus
What is the trend for ionization energy?
Increase from left to right across a period and decrease down a group
Decrease from left to right across a period and increase down a group
Stay constant within a period and increase down a group
Increase toward the center of the table
Circle the atom with the greater ionization energy: Si or Ag
Si
Ag
Circle the atom with the greater ionization energy: Ba or At
Ba
At
Circle the atom with the greater ionization energy: F or Cl
F
Cl
Circle the atom with the greater ionization energy: Pb or Sn
Pb
Sn
What is electron affinity?
The energy released when a neutral atom in the gas phase gains an electron
The energy required to remove an electron from a neutral atom
The tendency of an atom to attract electrons in a chemical bond
The number of electrons in the outermost shell
What is the trend for electron affinity?
It generally becomes more favorable across a period (left to right) and less favorable down a group
It generally becomes less favorable across a period (left to right) and more favorable down a group
It remains constant across periods and groups
There is no recognizable trend in the periodic table
What is electronegativity?
The tendency of an atom to attract shared electrons in a chemical bond
The energy released when an atom gains an electron
The energy required to remove an electron from an atom
The number of electrons in the valence shell
What is the trend for electronegativity?
It increases across a period (left to right) and decreases down a group
It decreases across a period (left to right) and increases down a group
It remains constant across the periodic table
It increases down a group and remains constant across a period
Circle the atom with the lower electronegativity: Na or K
Na
K
Circle the atom with the lower electronegativity: Cs or V
Cs
V
Circle the atom with the lower electronegativity: C or N
C
N
What is an ionic bond?
An electrostatic attraction between oppositely charged ions formed by the transfer of electrons
A sharing of electron pairs between atoms
A temporary attraction due to induced dipoles
A metallic lattice of delocalized electrons
What are valence electrons?
Electrons in the outermost energy level that participate in bonding
Electrons in inner shells that do not participate in bonding
Electrons emitted as radiation
Protons in the nucleus
What is a covalent bond?
A bond formed by sharing electron pairs between atoms
A bond formed by transferring electrons to create ions
A bond caused by metallic bonding
A bond caused by hydrogen attraction only
Draw the Lewis dot structure for the following atoms: Mg atom. How many dots should appear around the symbol for the Mg atom?
2
3
5
7
Draw the Lewis dot structure for the following atoms: N atom. How many dots should appear around the symbol for the N atom?
2
3
5
7
Draw the Lewis dot structure for the following atoms: F atom. How many dots should appear around the symbol for the F atom?
2
3
5
7
Draw the Lewis dot structure for the following atoms: Al. How many dots should appear around the symbol for the Al atom?
2
3
5
7
Draw the electron dot structure for the following cations: Ca ion. How many dots should appear around the symbol for the Ca ion in brackets?
0
2
4
8
Draw the electron dot structure for the following cations: Li-ion. How many dots should appear around the symbol for the Li ion in brackets?
0
2
4
8
Draw the electron dot structure for the following cations: B- ion. How many dots should appear around the symbol for the B⁻ ion in brackets?
0
3
4
8
Draw the electron dot structure for the following anions: S ion. Choose the description that matches the correct Lewis dot representation.
Eight dots around S with a 2− charge
Six dots around S with a 2+ charge
Seven dots around S with a 1− charge
Eight dots around S with a 1+ charge
Draw the electron dot structure for the following anions: Cl ion. Choose the description that matches the correct Lewis dot representation.
Eight dots around Cl with a 1− charge
Seven dots around Cl with a neutral atom
Eight dots around Cl with a 2− charge
Six dots around Cl with a 1+ charge
Draw the electron dot structure for the following anions: P ion. Choose the description that matches the correct Lewis dot representation.
Eight dots around P with a 3− charge
Five dots around P with a neutral atom
Eight dots around P with a 2− charge
Seven dots around P with a 1− charge
Draw the electron dot structures for the following ionic compounds: Magnesium and Chlorine. Select the correct compound formula and ion charges that satisfy octets.
MgCl2 with Mg2+ and two Cl−
MgCl with Mg+ and Cl−
Mg2Cl with Mg2+ and Cl−
MgCl3 with Mg3+ and three Cl−
Draw the electron dot structures for the following ionic compounds: Sodium and Iodine. Select the correct compound formula and ion charges that satisfy octets.
NaI with Na+ and I−
NaI2 with Na+ and two I−
Na2I with two Na+ and I2−
Na2I2 with two Na+ and two I−
Write the formula for the following ionic compounds: Copper (II) iodide.
CuI2
Cu2I
CuI
Cu2I2
Write the formula for the following ionic compounds: Lead (IV) nitride.
Pb3N4
PbN
Pb2N3
Pb4N3
Write the formula for the following ionic compounds: Aluminum nitride.
AlN
AlN3
Al3N2
Al2N
Write the name for the following ionic compounds: PbO2.
Lead(IV) oxide
Lead(II) oxide
Lead dioxide (molecular)
Plumbic oxide
Write the name for the following ionic compounds: Fe2O3.
Iron(III) oxide
Iron(II) oxide
Iron trioxide (molecular)
Ferric peroxide
Write the name for the following ionic compounds: KI.
Potassium iodide
Potassium(II) iodide
Potassium iodine
Potassium iodate
Write the formula for the following ternary ionic compounds: Sodium nitrate.
NaNO3
Na2NO3
NaNO2
NaN2O3
Write the formula for the following ternary ionic compounds: Calcium carbonate.
CaCO3
Ca(CO3)2
Ca2CO3
CaHCO3
Write the formula for the following ternary ionic compounds: Potassium sulfate.
K2SO4
KSO4
K2SO3
K3SO4
Write the formula for the following ternary ionic compounds: Iron(III) sulfate.
Fe2(SO4)3
FeSO4
Fe(SO4)2
Fe3(SO4)2
Write the correct name for each compound: Na2CO3.
Sodium carbonate
Sodium hydrogen carbonate
Sodium carbite
Sodium carbonite
Write the correct name for each compound: KNO3.
Potassium nitrate
Potassium nitrite
Potassium nitrogen trioxide
Potassium(III) nitrate
Write the correct name for each compound: Al(OH)3.
Aluminum hydroxide
Aluminum trihydrate
Aluminum(III) oxide
Aluminum hydrogen oxide
Write the correct name for each compound: Zn(OH).
Zinc hydroxide
Zinc(I) hydroxide
Zinc oxide
Zinc hydroxide monomer
