Download Chemical Bonding

Chemical Bonding
Name__________________________________Period:______Date:____________
CHEMICAL BONDS & VALENCE ELECTRONS
1) __________________________= an interaction between atoms that holds
them together by reducing the potential energy of their electrons
2) ____________________________= a shorthand representation of the
composition of a substance using atomic symbols and numeric subscripts (Ex:
NaCl, MgCl2, H2O, C6H12O6)
3) Chemical bonding involves the valence electrons of the atoms involved in
a___________________________.
4) _____________________________= the electrons available to be lost,
gained, or shared in the formation of chemical bonds
•
For atoms of main group elements, valance electrons are electrons in the
_______________________ main energy level.
•
Use of the periodic table to determine the number of valence electrons for
atoms of the main group elements:
Group
1
2
13
14
15
16
17
18
Number of Valence
Electrons
______________________= a helium atom has ________valence electrons
1
•
Electron Configuration of oxygen:
5) In the electron-dot formulas for atoms of main group elements, valence
electrons are represented by _________that surround an element’s symbol.
6) Examples of electron-dot formulas for atoms of the main group elements:
2
DETERMINING BOND TYPE
1)
__________________= a chemical bond resulting from
________________________________between positive and negative ions
a) In a purely ionic bond, one or more electrons are transferred from one atom
to another
2) _______________________= a chemical bond resulting from
the___________ of electrons between two atoms
a) ___________________= a covalent bond in which
the bonding electrons are ______________________
by the bonded atoms
b) ______________________= a covalent bond in
which the bonding electrons are ___________________
by the bonded atoms
δ+
δ-
3) Chemical bonds between two unlike atoms are NEVER
completely ionic and RARELY completely covalent. Bonds
can be anywhere in the range between these two extremes, depending upon
how strongly the bonded atoms attract electrons.
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4)
_______________________= a measure of the ability of an atom in
a chemical compound to attract electrons
5) The degree to which bonds are ionic or covalent can be ___________________
by comparing the electronegativities of the bonded atoms.
6) The electronegativity difference of two atoms can be used to determine the ionic
character of a bond.
•
Only ___________________values are used for the final electronegativity
7) The scale below can be used to classify the probable bond type between two
atoms.
a) If the electronegativity difference between two atoms is:
•
_________________the probable bond type is usually classified
as___________________________.
•
______________________the probable bond type is usually
classified as_______________________.
•
_____________________the probable bond type is usually classified
as __________________.
8) Polar covalent bonds, a closer look:
a) In a polar covalent bond electrons are________________________.
b) Shared electrons spend MORE of their time near the atom with the
_____________________ electronegativity.
c) __________________________ (δ+ or δ-) result.
ƒ
A δ- is assigned to the atom with the ________________electronegativity
ƒ
A δ+ is assigned to the atom with the ________________electronegativity
d) Ex: An H atom and a Cl atom form a polar-covalent bond resulting in partial
charges.
4
9) Determine the electronegativity difference and probable bond type with respect
to bonds formed between the following pairs of atoms. Assign partial charges if
the probable bond type is polar-covalent.
Pair of
Atoms
Electronegativity
Difference
Probable Bond
Type
Partial Charges
S and H
S and Cs
I and I
Cl and Br
S and Cl
Br and F
IONIC BONDING AND IONIC COMPOUNDS
1) Characteristics of ionic compounds:
a) Ionic compounds are held together by____________________________.
b) Ionic compounds usually involve__________________________________.
c) Ionic compounds are _____________under normal conditions.
d) Ionic compounds consist of a very large number of positive and negative ions
(anions and cations) that are combined so that the numbers of positive and
negative charges are________________.
e) The chemical formula for an ionic compound represents a formula unit, NOT
a____________________________.
2) An ionic compound is __________composed of independent, neutral units that
can be isolated and examined.
5
3) ____________________= a compound of positive and negative ions (anions
and cations) that are combined so that the numbers of positive and negative
charges are equal
4) The chemical formula of an ionic compound shows the _______of ions present
in a sample of any size.
a) Ex: magnesium chloride has the following chemical formula: MgCl2
ƒ
ƒ
For every one Mg+2 ion present, two Cl− ions are present.
If 13 mol Mg+2 ions are present in a sample, then 26 mol Cl− ions are
present in the sample.
5) The chemical formula for an ionic compound represents a formula unit, NOT a
molecule.
6) __________________= the simplest collection of atoms from which an ionic
compound’s formula can be established
7) __________________= chemical compounds tend to form so that each atom
(by gaining, losing, or sharing electrons) contains eight electrons in its
outermost occupied main energy level (valence electrons)
8) Electron-dot formulas can be used to illustrate the formation
of_________________.
a) Use electron-dot formulas to illustrate the formation of ionic bonds involving
Na and Cl.
6
b) Use electron-dot formulas to illustrate the formation of ionic bonds involving
Ca and F.
c) Use electron-dot formulas to illustrate the formation of ionic bonds involving K
and O.
COVALENT BONDING & MOLECULAR
SUBSTANCES
1) Characteristics of molecular substances:
a) Molecular substances are held together by___________________________.
b) Molecular substances usually involve ONLY ____________________.
c) Molecular substances may be ______________________________under
normal conditions.
d) Molecular substances consist of_______________________. The_________
of different molecules varies greatly.
2) _______________________= a chemical compound whose simplest units
are molecules
3) __________________= a neutral group of atoms held to together by
______________________________
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a) A single molecule is an individual unit capable of existing on its own.
4) The chemical formula for a molecular compound is called
a________________________.
5) _______________________________= a shorthand representation showing
the types and numbers of atoms combined in a single molecule
a) Ex: hydrogen peroxide; H2O2;________ atoms of hydrogen and _______
atoms of oxygen are held together by covalent bonds
b) Ex: glucose; C6H12O6; 6 atoms of carbon, 12 atoms of hydrogen, and 6
atoms of oxygen are held together by __________________
6) _______________________= a molecule containing only two atoms
a) Ex: HCl, O2
7) Certain elements occur naturally as diatomic molecules (you need to know
these elements!!)
a) They are: H2, O2, N2, Cl2, Br2, I2, and F2
8
ELECTRON-DOT FORMULAS AND
STRUCTURAL FORMULAS
1) Electron-dot formulas illustrate the sharing of ________________________
between atoms.
2) Electron pairs:
a) _________________= an electron pair NOT
involved in bonding
b) ______________= an electron pair shared
between two atoms
3) Types of covalent bonds:
a) ________________________= a covalent bond produced by the sharing of
one pair of electrons between two atoms
• Ex: H—H or H : H
b) ________________________= a covalent bond produced by the sharing of
two pairs of electrons between two atoms
•
Ex: O2
With six valence electrons each, two oxygen atoms
can use twelve electrons to satisfy both octets. By
sharing one electron from each oxygen, we can't
have more than one oxygen's octet satisfied. We'll
need to try a different sharing pattern; a double bond
will work.
c) ____________________= a covalent bond produced by the sharing of three
pairs of electrons between two atoms
• Ex: N2
With five valence electrons each, two nitrogen atoms
can use ten electrons to satisfy both octets. By sharing
one electron from each nitrogen, we can't have either
nitrogen's octet satisfied. We'll need to try a different
sharing pattern; a triple bond will work.
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d) In general, _________________are _________________and
____________than single bonds.
e) In general, __________________are shorter and stronger
than___________________.
4) Use electron-dot formulas to illustrate the formation of a Cl2 molecule from two
separate Cl atoms.
5) Guide for Writing Electron-Dot Formulas for Molecules:
a)
Count the ___________number of valence electrons in the molecule.
THESE ARE ALL THE ELECTRONS YOU MAY USE!
b)
Identify the central atom and terminal atoms:
ƒ
H is always a terminal atom
ƒ
C, if present is usually the _____________atom
ƒ
Molecules tend to be somewhat symmetrical (if one atom is different than
the others it is usually the central atom)
c)
Place _____________of electrons between each pair of bonded atoms to
form a____________________.
d)
Add electron pairs around the _____________________to satisfy the
octet rule for the terminal atoms. THERE ARE EXCEPTIONS TO THE
OCTET RULE! (see below)
e)
Assign left over electron pairs to the ___________________________.
f)
Orient atoms so there is _______________ electron pair repulsions around
the central atom. (arrange electron pairs as far apart as you can)
g)
If the central atom has LESS than an octet of electrons, then move one or
more lone pairs from the _________________atoms to form multiple bonds
(double and triple bonds).
ƒ
oxygen, nitrogen and carbon CAN form ___________________.
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h)
DO THE FOLLOWING FINAL CHECKS:
9 Check that the total number of valence electrons in the molecule is correct.
9 Check that the octet rule is satisfied for all atoms. DON’T FORGET
ABOUT THE EXCEPTIONS.
6) EXCEPTIONS to the octet rule:
a) _____________________is an exception to the octet rule. In a molecule,
hydrogen contains ________electrons in its outermost occupied main energy
level. HYDROGEN CAN FORM ONLY A SINGLE BOND AND WILL
CONTAIN NO LONE PAIRS!
b) ________________and _______________are SOMETIMES exceptions to
the octet rule. These atoms sometimes contain less than eight electrons in
their outermost occupied main energy level. Remembering that these atoms
DO NOT form double and triple bonds will be helpful when determining if
they break the octet rule.
7) Guide for Writing Structural Formulas for Molecules and Polyatomic
Ions:
a) Follow all guides from above except write a __________to indicate every
bond pair.
b) __________are still used to represent_________________.
8) Guide for Writing Electron-Dot Formulas for Polyatomic Ions:
a) Follow the guide from above except:
ƒ
Add a ____________and _______________to the electron-dot and
structural formulas
ƒ
Account for ______________when counting valence electrons
•
A POSITIVE CHARGE indicates you have to _____________electron(s)
o Ex: NH4 +1 has ____ valence electrons:
ƒ
N= _______________
ƒ
H4 = _____________
ƒ
So now there is _______ and you subtract ______since the
ion has a _____charge to get the final total of ___ valence
electrons
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o Ex: NH4 +1
_____________
____________
•
_____________
_____________
A NEGATIVE CHARGE indicates you have to _________electron(s)
o Ex: SO4-2 has _____valence electrons
ƒ
S= ________________________
ƒ
O4 = ________________________
ƒ
So now there is ________and you add _____since the ion
has a _____charge to get the final total of _____valence
electrons
THE VALENCE SHELL ELECTRON
PAIR REPULSION (VSEPR) MODEL
1) The _____________________has proven useful in
predicting molecular geometry and bond angles.
2) The VSEPR model assumes that atoms will orient
themselves so as to ___________electron pair repulsions
around the central atom.
3) Steps to determine molecular geometry and bond
angles:
a) Draw an electron-dot formula.
b) Arrange the electron pairs around the central atom in a
way that minimizes repulsion. In other words, put the
electron pairs as far apart as possible.
c) Determine molecular geometry:
d) Predict the bond angles from the molecular geometry.
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Molecular
Geometry
Atoms
Bonded
to
Central
Atom
Lone
Pairs
Around
the
Central
Atom
Predicted
Bond
Angles
Example
BeF2
2
0
BeF3
3
0
NH3
3
1
SnCl2
2
1
H2O
2
2
CH4
4
0
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e) Notice the bond angle distortion for molecules with a molecular geometry of
_____________________and ___________(with_____________________).
ƒ Ex: O3 is considered bent with a predicted bond angle of 120º since
there is only 1 lone pair of electrons
ƒ
Ex: H2O is considered bent with a predicted bond angle of 105° since
there is 2 lone pairs of electrons
ƒ
VSEPR model assumes that _______________require more room than
bond pairs and tend to compress the angles between bond pairs.
ƒ
In general, bond angles of at least _______________provide enough
room for lone pairs that significant bond angle distortion does NOT
occur.
™ Using The Modeling Kits:
ƒ
Easily shows molecular geometry
ƒ
A spring represents a single bond (one bond pair of electrons)
ƒ
A colored wooden ball represents various atoms
ƒ
When writing dot formulas and structural formulas you still will have to
account for lone pair(s) of electrons since models do not account for lone
pair(s)
Modeling Kit Color Code:
White = hydrogen
Black = carbon
Red = oxygen
Green = halogens
Orange = nitrogen
Yellow = sulfur
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POLAR vs. NONPOLAR MOLECULES
1) Use the following chart to determine if a molecule is polar or
nonpolar.
1.
Does the molecule have ANY polar bonds?
YES
NO
The molecule is NONPOLAR
2. Is the electronegativity of all terminal atoms the same?
NO
YES
The molecule is POLAR
Note: if the molecule
only contains 2 atoms,
stop after the first
question.
3. Is the molecule “symmetrical”?
(Lone pairs on central atom means molecule
is asymmetrical)
The molecule is POLAR
NO
YES
The molecule is NONPOLAR
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Complete the following tables as a class.
Formula
ICl
CH3I
BeF2
BF3
# of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
NA
Polar or
Nonpolar?
16
Formula
CO2
H2CO
NH3
H 2O
# of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
Polar or
Nonpolar?
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Formula
# of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
Polar or
Nonpolar?
NA
SO2
SO4−2
NA
NA
NH4+
N2
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Valence Electrons & Electron-Dot Notation Worksheet
1) Determine the number of valence electrons in one atom of each of the following
elements. Also, write the electron-dot notation for each element.
a) Na
b) F
c) Rb
d) Ba
e) I
f) Se
g) Al
h) C
i) Mg
j) Si
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Electronegativity & Probable Bond Type Worksheet
1) Determine the electronegativity difference and probable bond type with respect
to bonds formed between the following pairs of atoms. Assign partial charges if
the probable bond type is polar-covalent.
Pair of
Atoms
Electronegativity Difference
Probable Bond
Type
Partial Charges (if
polar-covalent)
H and H
S and O
H and I
K and Br
Si and Cl
H and F
Se and S
C and H
Na and Cl
O and H
N and N
I and Cl
20
Ionic Bonding & Ionic Compounds Worksheet
1) Use electron-dot formulas to illustrate the formation of ionic bonds involving
Li and Cl.
2) Use electron-dot formulas to illustrate the formation of ionic bonds involving
Ca and I.
3) Use electron-dot formulas to illustrate the formation of ionic bonds involving
K and F.
4) Use electron-dot formulas to illustrate the formation of ionic bonds involving
Mg and Br.
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5) Use electron-dot formulas to illustrate the formation of ionic bonds involving
Al and I.
6) Use electron-dot formulas to illustrate the formation of ionic bonds involving
Ca and O.
7) Use electron-dot formulas to illustrate the formation of ionic bonds involving
Na and S.
8) Use electron-dot formulas to illustrate the formation of ionic bonds involving
Al and S.
22
Complete the following table.
Formula
NO2+
O3
BF4−
H2BF
Number
of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
Polar or
Nonpolar?
NA
NA
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Formula
BeCl2
CH4
NO2−
HCl
Number
of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
NA
Polar or
Nonpolar?
NA
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Formula
Cl2CO
CHCl3
NF3
CCl4
Number
of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
Polar or
Nonpolar?
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Formula
H2
CHI3
H2Te
SiO2
Number
of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
NA
Polar or
Nonpolar?
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Formula
H 2S
HCN
ClO−
PH3
Number
of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
NA
Predicted
Bond
Angles
NA
Polar or
Nonpolar?
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Formula
ClO2−
HClO
PCl3
OF2
Number
of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
Polar or
Nonpolar?
NA
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Formula
H 3 O+
I2
CF4
SCl2
Number
of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
NA
Polar or
Nonpolar?
NA
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Formula
NCl3
Cl2O
NH2Cl
SiCl3Br
Number
of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
Polar or
Nonpolar?
30
Formula
ONCl
NO3−
SO4−2
SCN−
Number
of
Valence
Electrons
Electron-Dot Formula
Structural Formula
Molecular
Geometry
Predicted
Bond
Angles
Polar or
Nonpolar?
NA
NA
NA
31
IONIC COMPOUNDS
MOLECULAR COMPOUNDS
Ionic Compounds vs. Molecular Compounds
1. What type(s) of elements are usually contained in this type of compound? 2. Under ordinary conditions, in what state of matter would you find this compound? 3. This type of compound can be described as a collection of ________? 4. What type of bond is holding the atoms together? Explain how atoms are held together by this type of bonding? 32
Bonding Basics Worksheet
Vocabulary: Use your notes to help you identify the following vocabulary.
1) A __________________________________is a covalent bond produced by the sharing of two pairs of
electrons between two atoms
2) ____________________________is a measure of the ability of an atom in a chemical compound to attract
electrons
3) _________________________ is a chemical bond resulting from electrostatic attraction between
positive & negative ions
4) A _________________ is a neutral group of atoms held to together by covalent bonds
5) __________________________ is a chemical bond resulting from the sharing of electrons between
two atoms
6) A _____________________________ is a covalent bond produced by the sharing of three pairs of
electrons between two atoms
7) ___________________________ is a covalent bond in which the bonding electrons are shared
unequally by the bonded atoms
8) A _________________________is a molecule containing only two atoms
9) _______________________________ is an electron pair shared between two atoms
10) _____________________________ is an interaction between atoms that holds them together by
reducing the potential energy of their electrons
11) _______________________________is the simplest collection of atoms from which an ionic
compound’s formula can be established
12) ____________________________is a shorthand representation of the composition of a substance
using atomic symbols and numeric subscripts (Ex: NaCl, MgCl2, H2O, C6H12O6)
13) ______________________________ is the tendency of compounds to form so that each atom (by
gaining, losing, or sharing electrons) contains eight electrons in its outermost occupied main energy
level (valence electrons)
14) A ____________________________is a chemical compound whose simplest units are molecules
15) _____________________________ is the outermost electrons available to be lost, gained, or shared
in the formation of chemical bonds
16) _______________________________ is an electron pair NOT involved in bonding
17) __________________________ is a covalent bond in which the bonding electrons are shared equally
by the bonded atoms
18) A ______________________________ is a covalent bond produced by the sharing of one pair of
electrons between two atoms
19) _____________________________ is the atom in the center of the compound, often carbon
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Concepts: Answer the following questions.
1. When predicting probable bond types, list the ranges for the following:
a. Non-polar covalent =______________________________
b. Polar-covalent = __________________________________
c. Ionic = __________________________________________
2. Which atom is assigned the partial negative charge?
3. Ionic compounds contain what type of elements?_____________________________________
4. What phase(s) of matter would you most likely find ionic compounds? _______________________
5. Molecular substances usually involve only what type of elements? __________________________
6. What phase(s) of matter would you most likely find molecular compounds? _____________________
7. List the naturally occurring diatomic molecules.
________________________________________________________________
8. What are the 3 exceptions to the octet rule when constructing electron dot formulas?
9.
Use electron dot formulas to illustrate the formation of ionic bonds involving Li and N.
10. Use electron dot formulas to illustrate the formation of ionic bonds involving Na and O.
34
Dot & Structural Formulas: For each of the following formulas determine the number of valence electrons and
draw the electron dot formula and structural formula.
Number
of
Formula Valence Electron Dot Formula
Electrons
Structural Formula
PH3
SO3
CS2
CH2O
SiCl4
(silicon
tetrachloride)
35
BONDING REVIEW WORKSHEET
1) What are valance electrons?
a. Where are valance electrons found?
2) What is an ionic bond?
3) What is the difference between a non-polar covalent bond and a polar-covalent
bond?
4) What is electronegativity?
5) When predicting probable bond types, list the ranges for the following:
a. Non-polar covalent =______________________________
b. Polar-covalent = __________________________________
c. Ionic = __________________________________________
6) Which atom is assigned the partial negative charge?
7) Ionic compounds contain what type of elements? _________________________________
8) What phase(s) of matter would you most likely find ionic compounds?
9) What is the octet rule?
10)Molecular substances usually involve only what type of elements?__________________
11)What phase(s) of matter would you most likely find molecular compounds?
36
12)What are diatomic molecules? List the naturally occurring diatomic molecules.
13)What is the difference between lone pair electrons and bond pair electrons?
14)What are the exceptions to the octet rule when constructing electron dot formulas?
15)What needs to be added to the electron dot and structural formulas for polyatomic
ions? __________________________ & ______________________________
16)List the 6 types of molecular geometry that a compound may exhibit and the
predicted bond angle.
17) Use electron dot formulas to illustrate the formation of ionic bonds involving Ca and
Cl.
18)Use electron dot formulas to illustrate the formation of ionic bonds involving K and O.
37
Unit Learning Map (10 days):
Class:
Bonding
Mrs. Hostetter
Academic Chemistry A - Grade 11
Unit Essential Question(s):
Optional
Instructional Tools:
Why is one atom rarely
found by itself in
nature?
Concept
Chemical Bonds
Lesson Essential Questions:
Why do chemical bonds
form?
Vocabulary:
Chemical bond
Chemical formula
Valence electrons
Concept
Bond Types
Lesson Essential Questions:
How do you determine
probably bond type?
Vocabulary:
Ionic bonds
Covalent bond
Nonpolar-covalent bond
Polar-covalent bond
Electronegativity
Ionic compound
Formula unit
Octet rule
Molecular compound
Molecule
Molecular formula
Diatomic molecule
Guided Notes
Lab Materials:
ƒ
ƒ
Modeling Lab
Ionic Compound Lab
Concept
Electron Dot and Structural
Formulas
Concept
VSEPR Model
Lesson Essential Questions:
Lesson Essential Questions:
How can molecules and
polyatomic ions be
represented using electron
dot and structural formulas?
How can the VSEPR model
be used to predict molecular
geometry and bond angles?
Vocabulary:
Lone pair electrons
Bond pair electrons
Single bond
Double bond
Triple bond
Central atom
Dot formula
Structural formula
Vocabulary:
VSEPR Model
Molecular geometry
Bond angles
Linear
Trigonal planar
Bent
Tetrahedral
Trigonal Pyramidal
38
Bonding Vocabulary:
20) Chemical bond- an interaction between atoms that holds them together by reducing the potential
energy of their electrons
21) Chemical formula- a shorthand representation of the composition of a substance using atomic
symbols and numeric subscripts (Ex: NaCl, MgCl2, H2O, C6H12O6)
22) Valence electrons- the outermost electrons available to be lost, gained, or shared in the formation of
chemical bonds
23) Ionic bonds- a chemical bond resulting from electrostatic attraction between positive & negative ions
24) Covalent bonds- a chemical bond resulting from the sharing of electrons between two atoms
25) Nonpolar-covalent bond- a covalent bond in which the bonding electrons are shared equally by the
bonded atoms
26) Polar-covalent bond- a covalent bond in which the bonding electrons are shared unequally by the
bonded atoms
27) Electronegativity- a measure of the ability of an atom in a chemical compound to attract electrons
28) Ionic compound- a compound of positive and negative ions (anions and cations) that are combined so
that the numbers of positive and negative charges are equal
29) Formula unit- the simplest collection of atoms from which an ionic compound’s formula can be
established
30) Octet rule- chemical compounds tend to form so that each atom (by gaining, losing, or sharing
electrons) contains eight electrons in its outermost occupied main energy level (valence electrons)
31) Molecular compound- a chemical compound whose simplest units are molecules
32) Molecule- a neutral group of atoms held to together by covalent bonds
33) Molecular formula- a shorthand representation showing the types and numbers of atoms combined in
a single molecule
34) Diatomic molecule- a molecule containing only two atoms (Natural = H2,O2, N2, Cl2, Br2, I2, F2)
35) Lone pair electrons- an electron pair NOT involved in bonding
36) Bond pair electrons- an electron pair shared between two atoms
37) Single bond- a covalent bond produced by the sharing of one pair of electrons between two atoms
38) Double bond- a covalent bond produced by the sharing of two pairs of electrons between two atoms
39) Triple bond- a covalent bond produced by the sharing of three pairs of electrons between two atoms
40) Central atom- atom in the center of the compound, often carbon
41) Dot formula- when dots are used to show bond pairs and lone pairs
42) VSEPR Model- (Valence Shell Electron Pair Repulsion Model) has proven useful in predicting
molecular geometry and bond angles
43) Molecular geometry- Linear, Trigonal planer, Bent, Tetrahedral, Trigonal pyramidal, and Bent
44) Bond angles- angle at which the bond takes place
45) Linear- 2 atoms bonded to central angle and predicted bond angles is 180°
46) Trigonal planar- 3 atoms bonded to central angle and predicted bond angles is 120°
47) Bent- 2 atoms bonded to central angle, 1 lone pair around the central atom; predicted bond angle is
120°
48) Bent- 2 atoms bonded to central angle, 2 lone pairs around central atom; predicted bond angle is 105°
49) Tetrahedral- 4 atoms bonded to central angle; predicted bond angle is 109.5°
50) Trigonal Pyramidal- 3 atoms bonded to central angle, 1 lone pair around central atom; predicted
bond angle is 107°
39