Ionic, Metallic and Covalent Bonding

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Ionic, Metallic and Covalent Bonding Writing and
Naming Formulas
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Chemical bond
force that holds two atoms together
opposites attract
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Chemical bonds are formed by
the attraction between the positive nucleus of
one atom and the negative electrons of another
atom
or by the attraction between positive and
negative ions
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Krypton
Potassium in water
Iron in oxygen
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Valence electrons
electrons available to be lost, gained, or shared
in the formation of chemical compounds
found in outermost energy level
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oct
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Octet Rule
Atoms tend to gain, lose, or share electrons in
order to acquire a full set of eight valence
electrons stable noble gas configuration.
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Three types of bonds

• Ionic
• transfer of electrons between
• metal and nonmetal (or
• polyatomic ion)

2. Metallic electron sea model atoms
of same metal
3. Covalent sharing of electrons between
nonmetals may be same or different elements
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Ion
atom, or a bonded group of atoms, that has a
positive or negative charge
Ionic bond
electrostatic force that holds oppositely charged
particles together
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Positive ion formation
atom loses one or more valence electrons
cations
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Write an electron configuration for sodium.
Write an electron configuration for neon.
What is the only difference in the electron
configurations of these two elements?
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Metals tend to lose electrons to form positive
ions called cations.
Metals lose all valence electrons so that next
energy level is full.
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Write an electron dot notation for each metal
Magnesium Aluminum Lithium Barium Potassium Galliu
m
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Predict if each would lose or gain electrons when
forming compounds
Magnesium Aluminum Lithium Barium Potassium Galliu
m
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How many electrons would each lose?
Magnesium Aluminum Lithium Barium Potassium Galliu
m
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What cations would the following elements form?
Write symbol and charge.
Magnesium Aluminum Lithium Barium Potassium Galliu
m
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Use group number to predict charge of metal ion
for representative elements only.
Group 1 1
Group 2 2
Group 13 3
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Transition metals
d block filling inner energy levels
most form more than one common ion
sometimes inner electrons take part in bonding
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Transition metals that form only one common ion
silver Ag
zinc Zn2
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Negative ion formation
atom gains one or more valence electrons
anion
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Write an electron configuration for chlorine.
Write an electron configuration for argon.
What is the only difference in the electron
configurations of these two elements?
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Nonmetals tend to gain electrons to form negative
ions called anions.
Nonmetals gain enough electrons to obtain full
octet (8).
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Write an electron dot notation for each nonmetal
Sulfur Nitrogen Iodine Phosphorus Fluorine Oxygen
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Predict if each would lose or gain electrons when
forming compounds
Sulfur Nitrogen Iodine Phosphorus Fluorine Oxygen
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How many electrons would each gain?
Sulfur Nitrogen Iodine Phosphorus Fluorine Oxygen
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What anions would the following elements
form? Write symbol and charge.
Sulfur Nitrogen Iodine Phosphorus Fluorine Oxygen
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Use group number to predict charge on nonmetals.
Group 18 0
Group 17 1-
Group 16 2-
Group 15 3-
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Writing formulas for binary ionic compounds

• Write symbol and charge for
• cation and anion.

Ex lithium and oxygen
2. Use subscripts to show the ratio of ions.
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Cation always written first.
Ionic formulas, subscripts show simplest ratio.
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Write formulas for the binary ionic
compounds formed between the following elements

1. potassium and iodine

b. magnesium and chlorine
c. sodium and sulfur
d. aluminum and nitrogen
e. aluminum and sulfur
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Naming binary ionic compounds
cation (metal) name of element always
written first
anion (nonmetal) name of element with an
ide ending
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Name the binary ionic compounds indicated by
the following formulas

1. AgCl
2. ZnO
3. CaBr2
4. SrF2
5. BaO
6. CaCl2

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Some metals form more than one common ion most
of the transition metals and tin and lead.
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How form multiple ions?
Transition metals d electrons can take part in
bonding
Write noble gas notation for tin
Kr 5s24d105p2
Sn2 or Sn4
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The charge on the metal is written as a Roman
numeral in the name of compound.
Fe2 Cl-
FeCl2
iron(II) chloride
Fe3 Cl-
FeCl3
iron(III) chloride
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Transition metals that form only one common ion
silver Ag
zinc Zn2
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Metals that form only one common ion do not need
Roman numeral.
NaBr sodium bromide
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Write the formula and name for the compounds
formed between the following ions (use Roman
numerals)

1. Cu2 and Br -
2. Fe2 and O2-
3. Pb2 and Cl-
4. Hg2 and S2-
5. Sn2 and F-
6. Fe3 and O2-

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Writing names with Roman numerals

• Determine total negative
• charge.

2. Total negative charge equals total
positive charge.

• Charge on one positive ion is
• Roman numeral.

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Ionic compounds containing polyatomic ions
Write formulas as you would for binary ionic
compounds use parentheses if adding subscript
to polyatomic ion.
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Write formulas for the following compounds
magnesium carbonate
magnesium hydroxide
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Write formulas for the following ionic compounds

1. lithium nitrate
2. copper(II) sulfate
3. sodium carbonate
4. calcium nitrite
5. potassium perchlorate

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When naming compounds, do not change name
of polyatomic ion.
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Three types of bonds

• Ionic
• transfer of electrons between
• metal and nonmetal (or
• polyatomic ion)

2. Metallic electron sea model atoms
of same metal
3. Covalent sharing of electrons between
nonmetals may be same or different elements
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Why do atoms bond?
to obtain a full outer energy level complete
octet
to become more stable lower potential energy
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Electronegativity (EN)
indicates relative ability of an atom to attract
electrons in a chemical bond
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Metals
low EN tend to give up electrons
Nonmetals
high EN tend to gain electrons
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What happens when two nonmetals, with similar EN,
react?
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Covalent bond
chemical bond that results from the sharing of
valence electrons
generally formed between two nonmetals (same or
different element)
electrons are attracted by the nuclei of two
different atoms
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Molecule
formed when two or more atoms bond covalently
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Naming binary molecular compounds

• First element use entire
• element name.

2. Second element ends in ide.

• Prefixes are used to indicate
• the number of atoms of each
• element the subscripts.

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N2O4
dinitrogen tetroxide
If first element has one atom, mono omitted.
CO
carbon monoxide
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Name the following molecular compounds

1. PF3
2. XeF4
3. As2O5
4. CCl4

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Write formulas for the following compounds

1. carbon dioxide
2. dinitrogen pentoxide
3. silicon tetrafluoride

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Ionic compounds composed of large
numbers of cations and anions crystal lattice
formula unit smallest whole number ratio of
ions
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Molecular compounds composed of discrete
(individual) molecules of covalently
bonded atoms
molecular formulas do not need to be lowest ratio
of atoms
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C2H4
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Acid
a substance that produces hydrogen ions
(H) when dissolved in water
molecular compound that reacts with water to form
ions
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• binary acid two elements
• hydrogen and a nonmetal

name begins with prefix hydro and ends with ic
hydrochloric acid
HCl
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• oxyacid hydrogen, oxygen,
• and a nonmetal many formed
• from polyatomic ions

if name of polyatomic ion ends with ate , name
of acid ends with ic
H2SO4
sulfuric acid
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Binary acid hydro _____ ic acid Oxyacid
______ ic acid
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Name the following acids
H2CO3
HBr
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Writing formulas for acids
start with H
determine charge on nonmetal ion or polyatomic
ion
add subscripts if needed to make neutral compound
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Write formulas for the following acids
hydrofluoric acid
phosphoric acid
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Electronegativity (EN)
indicates the relative ability of an atom to
attract electrons in a chemical bond
Type of bond formed between two atoms depends on
the difference in electronegativities (DEN) of
the atoms.
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Difference in electronegativity (DEN)
locate elements on periodic table
subtract values for EN
DEN always positive
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Ex hydrogen and chlorine
DEN 3.16 2.20 0.96
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Covalent bonds may be
Polar covalent bond
unequal sharing of electrons
one atom pulling electrons towards itself
atom with higher EN value has a partial negative
charge (d-)
atom with lower EN value has a partial positive
charge (d)
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Ex hydrogen and chlorine
DEN 3.16 2.20 0.96
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Covalent bonds may be
Nonpolar covalent bond electrons shared
equally no partial charges
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Most bonds are not completely ionic or covalent.
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DEN Bond Character
gt 1.7 Ionic
0.4 1.7 polar covalent
lt 0.4 nonpolar covalent
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Classify the following bonds as nonpolar-
covalent, polar-covalent, or ionic. If bond is
polar-covalent, assign partial charges.
C and H
H and Br
Cs and S
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Properties of Compounds depend on the
strength of the attractive forces between
particles
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Properties of ionic compounds
ions arranged in a regular repeating pattern
called crystal lattice
ions held together by strong ionic bonds
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Properties of ionic compounds
high melting and boiling points much energy
needed to separate ions
hard, rigid, brittle solids
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Properties of ionic compounds
do not conduct electricity in solid state
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aqueous solutions and liquid states are
electrolytes - conduct electricity since ions
are free to move
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Properties of molecular compounds covalent
bonds between atoms are strong, but attraction
forces between molecules are weak
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Intermolecular forces
relatively weak forces of attraction between
molecules
also known as van der Waals forces
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Properties of molecular compounds
relatively low melting and boiling points many
gases or liquids at room temperature
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Properties of molecular compounds
do not conduct electricity when dissolved in
water except for acids
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Metallic bond
outer energy levels of metal atoms overlap
valence electrons are shared by several atoms
delocalized (free to move)
electron sea model
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Metallic bond
attraction of a metallic cation for delocalized
electrons
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Properties of metals
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Properties of metals
moderately high melting points and high boiling
points most solids are room temperature
the more delocalized electrons a metal has, the
greater its strength and hardness groups 1 2
soft
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Metals are malleable (hammered into thin sheets)
and ductile (drawn into wires.)
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good conductors of heat and electricity
electrons mobile
delocalized electrons interact with light, giving
metals luster (shiny)
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Three types of bonds

• Ionic transfer of e-
• metal and nonmetal

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2. Metallic electron sea model atoms
of same metal
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3. Covalent sharing of e- nonmetals
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• Nonpolar Covalent - no charges
• Polar Covalent - partial charges

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James
Bond