[GENERAL CHEMISTRY] Bonds in Chemistry

Proverbs 16:3

a. Molecule

[CHEMICAL BONDS]

Aggregate of 2 or more atoms in definite arrangement held together by chemical bonds.

a. Molecule

b. Compound

c. Ions

d. Electrode

e. Empirical formula

f. Molecular formula

c. Ions

[CHEMICAL BONDS]

With net (+) or (-) charge.

a. Molecule

b. Compound

c. Ions

d. Electrode

e. Empirical formula

f. Molecular formula

e. Empirical formula

Example: The Empirical formula of C6H₁₂O₆ is CH₂O.

[CHEMICAL BONDS]

Simplest whole number ratio.

a. Molecule

b. Compound

c. Ions

d. Electrode

e. Empirical formula

f. Molecular formula

a. True

[CHEMICAL BONDS]

Empirical formula cannot be the same with molecular formula.

a. True

b. False

f. All

Intermolecular force of attraction is also known as Van der Waals and Electrostatic

[FORCES OF ATTRACTION]

Forces of attraction between molecules.

a. Intermolecular

b. Van der Waals

c. Electrostatic

d. a and b

e. b and c

f. All

d. Intramolecular force of attraction

[FORCES OF ATTRACTION]
Forces of attraction within molecules.

a. Intermolecular

b. Van der Waals

c. Electrostatic

d. Intramolecular

e. a and b

f. c and d

a. I, II, III

[FORCES OF ATTRACTION]
Intermolecular forces of attraction:

I. Van der Waals or Electrostatic

II. Created by molecule's polarizability

III. Exerted when 2 uncharged atoms (n⁰) approach very closely

a. I, II, III

b. I, II

c. I, III

d. II, III

c. Ionic - this is an INTRAmolecular force.

[FORCES OF ATTRACTION]

Intermolecular forces of attraction except:

a. H-bonding

b. Keesom orientation

c. Ionic

d. Debye Induction

e. London Dispersion

f. None

a. H-bonding

[FORCES OF ATTRACTION]
Strongest intermolecular force of attraction.

a. H-bonding

b. Keesom orientation

c. Debye Induction

d. London Dispersion

a. H-bonding

[FORCES OF ATTRACTION]
Include electronegative atoms such as H+ S, O, N, X (F, Cl, Br, I).

a. H-bonding

b. Keesom orientation

c. Debye Induction

d. London Dispersion

b. Keesom orientation (D-D)

[FORCES OF ATTRACTION]
Involves dipole-dipole or water-water which are polar to polar.

a. H-bonding

b. Keesom orientation

c. Debye Induction

d. London Dispersion

c. Debye Induction (D-ID)

Tips to remember:

• Debye is D-ID: Debye sound like DIDBye.

[FORCES OF ATTRACTION]
Involved dipole-induced dipole or water-benzene which are polar to non-polar.

a. H-bonding

b. Keesom orientation

c. Debye Induction

d. London Dispersion

d. London Dispersion

[FORCES OF ATTRACTION]
Weakest intermolecular force of attraction.

a. H-bonding

b. Keesom orientation

c. Debye Induction

d. London Dispersion

d. London Dispersion (ID-ID)

[FORCES OF ATTRACTION]

Involved induced dipole-induced dipole, benzene-benzene, or aromatics which are non-polar to non-polar.

a. H-bonding

b. Keesom orientation

c. Debye Induction

d. London Dispersion

d. H-bonding -> Keesom orientation -> Debye Induction -> London Dispersion

[FORCES OF ATTRACTION]
Arrange from strongest to weakest IFA.

a. London Dispersion -> Debye Induction -> Keesom orientation -> H-bonding

b. London Dispersion -> Keesom orientation -> Debye Induction -> H-bonding

c. H-bonding -> Debye Induction -> Keesom orientation -> London Dispersion

d. H-bonding -> Keesom orientation -> Debye Induction -> London Dispersion

a. True

Keesom is dipole-dipole while debye is dipole-induced dipole.

[FORCES OF ATTRACTION]
Keesom orientation is a stronger IFA than Debye Induction.

a. True

b. False

e. None

• Covalent is involved in nonmetal + nonmetal

• Ionic is involved in metal + nonmetal

[FORCES OF ATTRACTION]

Intramolecular force of attraction except:

a. Covalent

b. Ionic

c. Nonmetal + Nonmetal

d. Metal + Nonmetal

e. None

f. All

Tips to remember:

• Covalent bonding is sharing of electron: "Co" = share

[FORCES OF ATTRACTION]

Covalent Intramolecular FA:

a. Sharing of electron

b. Nonmetal + nonmetal

c. Glycosidic and peptide bond

d. a and b

e. b and c

f. All

a. Glycosidic

[FORCES OF ATTRACTION]
Ether bond: S-O-S.

a. Glycosidic

b. Peptide bond

c. Ionic bond

b. Peptide bond

[FORCES OF ATTRACTION]
Amide bond: AA-peptide-AA.

a. Glycosidic

b. Peptide bond

c. Ionic bond

f. All

[FORCES OF ATTRACTION]
Ionic bond

a. Transfer of e-

b. Metal + Nonmetal

c. Involved in NaCl

d. a and b

e. b and c

f. All

a. Lone pair

[FORCES OF ATTRACTION]
Pair of valence electrons that are not shared with another atom in covalent bond.

a. Lone pair

b. Valence pair

c. Lone valence

d. Valence free

a. Valence shell electron pair repulsion (VSEPR) theory

[FORCES OF ATTRACTION]

Predicts the geometry of the molecule as well as any bonded and unbonded electron pair.

a. Valence shell electron pair repulsion (VSEPR) theory

b. Valence bond theory

c. Molecular orbital theory

a. 180°

[FORCES OF ATTRACTION]
Angle of linear VSEPR geometry:

a. 180°

b. 120°

c. 109.5°

b. 120°

[FORCES OF ATTRACTION]
Angle of trigonal planar VSEPR geometry:

a. 180°

b. 120°

c. 109.5°

c. 109.5°

[FORCES OF ATTRACTION]

Angle of tetrahedral/bent VSEPR geometry:

a. 180°

b. 120°

c. 109.5°

a. Linear VSEPR geometry

[FORCES OF ATTRACTION]
Alkynes (Sp)

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

a. Linear VSEPR geometry

[FORCES OF ATTRACTION]
CO2

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

b. Trigonal planar VSEPR geometry

[FORCES OF ATTRACTION]
Alkenes (Sp2 )

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

b. Trigonal planar VSEPR geometry

[FORCES OF ATTRACTION]
120°

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

b. Trigonal planar VSEPR geometry

[FORCES OF ATTRACTION]
Formaldehyde

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

d. Trigonal VSEPR geometry

PF5 (Phosphorus pentafluoride)

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

b. Trigonal planar VSEPR geometry

[FORCES OF ATTRACTION]

BF3 (Boron trifluoride)

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

[FORCES OF ATTRACTION]

Alkanes (Sp3)

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

[FORCES OF ATTRACTION]

109.5°

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

[FORCES OF ATTRACTION]

2 bonded pair, 2 unbonded pair.

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

[FORCES OF ATTRACTION]
CCl₄ (Carbon tetrachloride)

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

[FORCES OF ATTRACTION]
H₂O (Water)

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

[FORCES OF ATTRACTION]

Methane

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

d. Trigonal Bipyramidal VSEPR geometry

[FORCES OF ATTRACTION]
107°

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal Bipyramidal VSEPR geometry

e. Octahedral VSEPR geometry

e. Octahedral VSEPR geometry

[FORCES OF ATTRACTION]
SF5

a. Linear VSEPR geometry

b. Trigonal planar VSEPR geometry

c. Tetrahedral/bent VSEPR geometry

d. Trigonal VSEPR geometry

e. Octahedral VSEPR geometry

e. b and c - trigonal and octahedral

[FORCES OF ATTRACTION]
VSEPR geometry exempted to the octet rule:

a. Tetrahedral

b. Trigonal

c. Octahedral

d. a and b

e. b and c

f. All

b. Valence bond theory

[FORCES OF ATTRACTION]
States that bonds are formed by sharing of electron from overlapping atomic orbitals (covalent)

a. Valence shell electron pair repulsion (VSEPR) theory

b. Valence bond theory

c. Molecular orbital theory

f. All

[FORCES OF ATTRACTION]
Spherical shape:

a. Sigma bond

b. Stronger bond formed

c. Headways overlap

d. a and b

e. b and c

f. All

f. All

[FORCES OF ATTRACTION]

Dumbbell shape:

a. Pi bond

b. Weaker bond formed

c. Sideways overlap

d. a and b

e. b and c

f. All

c. Molecular orbital theory

[FORCES OF ATTRACTION]

States that bonds are formed from interaction of atomic orbitals from molecular orbitals.

a. Valence shell electron pair repulsion (VSEPR) theory

b. Valence bond theory

c. Molecular orbital theory

c. Both

[FORCES OF ATTRACTION]
Bonding:

a. Lower energy

b. Stable

c. Both

d. None

c. Both

[FORCES OF ATTRACTION]
Anti-bonding

a. Higher energy

b. Unstable

c. Both

d. None