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Chemistry > Bonding > Flashcards

Bonding Flashcards

1
Q

Atom

A

Smallest particle that characterizes a chemical element

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2
Q

Octet Rule

A

When bonds form between atoms, the atoms gain, lose, or share electrons in a way that they create outer energy levels w/ 8 electrons

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3
Q

Bonding occurs when….where….why…

A

Valence electrons are shared or transferred at the highest energy level to make it more stable
- Electrons in lower energy lvls are not involved w/ bonding

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4
Q

Define orbitals

A

Space around an atoms nucleus where an electron may exist

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5
Q

Define Valence Orbitals

A

Volume of space that can be occupied by electrons in atoms highest energy lvl (outer layer)

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6
Q

Define Bonding Electrons

A

Un-paired electrons that can be shared w/ other atoms

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7
Q

Define Lone Pair

A

Two electrons occupying same orbital

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8
Q

Define Valence Electrons

A

Electrons in highest energy lvl in atom

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9
Q

Define Ionic Bond

A

Attraction between pos. and neg. ions resulting in transfer of one or more valence electrons

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10
Q

Define Covalent Bond

A

Two or more electrons are shared among the atoms

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11
Q

Which bond is stronger, (covalent or ionic)

A

Ionic is stronger

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12
Q

Define Electronegativity

A

Ability of atom to attract pair of bonding electrons in valance lvl
- Increase as you go up or right of the periodic table

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13
Q

Define Non-polar Molecule

A

A molecule w/ symmetrical electron distribution

NOTE: Hydrocarbons are always non-polar

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14
Q

Define Polar Molecule

A

Molecule in which negative charges are not distributed symmetrically among atoms causing partial negative and partial positive charge on both sides of atom

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15
Q

Electronegativity for ionic compound

A

Difference in electronegativities is usually greater than 1.7 causing electrons to be transferred.

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16
Q

Difference in Electronegativity (DEN)

A

DEN = 0 - Nonpolar covalent bond
DEN between 0.1-1.7 - Polar Covalent bond
DEN between 1.7-4 - Ionic bond

17
Q

Bond Dipole

A

When arrow points towards more electronegativity end of compound

18
Q

Define Intramolecular Forces

A
  • Forces within the molecule

- Responsible for physical behaviour of molecule substance

19
Q

What are the two types of intramolecular forces?

A
  1. Ionic Bonds: within crystal lattice

2. Covalent Bonds: within a molecule

20
Q

Define Intermolecular Forces

A
  • Forces between molecules
  • Responsible for physical properties in molecules
  • Present between covalent compunds
21
Q

Types of Intermolecular Forces

A
  1. Van der Waals Forces
    - London Dispersion Forces
    - Dipole-Dipole Forces
  2. Hydrogen Bonding
22
Q

London Dispersion Forces

A
  • Always present between all molecules, does not matter if there are different attractions
  • Any electron movement within molecule can produce momentary dipole
  • Force gets stronger as # of electrons in molecule increases
  • More electrons = more LDF
23
Q

Relationship between Boiling point and Intermolecular bonds

A
  • Stronger LDF = greater strength of intermolecular forces

- Greater strength of intermolecular forces = higher BP of substance

24
Q

Dipole - Dipole Forces

A
  • Exist between polar bonds ONLY

- Strength of Dipole force is dependent on overall polarity, more polar = greater DD force

25
Q

Hydrogen Bonding

A
  • Strongest intermolecular force
  • Only occurs when hydrogen bonds to: Oxygen, Nitrogen, or Fluorine
  • Must have at least one lone pair
26
Q

Intermolecular forces of non-polar molecule, polar molecule, and polar molecule w/ H bonded w/ N,O, F

A

Non-polar = LDF
Polar = LDF, DD
Polar w/ H bonded N,O, F = LDF, DD, HB

27
Q

List the strengths of attractions for intermolecular and intramolecular forces (weakest to strongest)

A
  1. LDF
  2. DD
  3. HB
  4. Covalent Compounds
  5. Ionic compunds
28
Q

What does VSEPR stand for

A

Valence Shell Electron Pair Repulsion Theory

29
Q

Shape of AXE3 and polarity

A
  • Linear
  • 2 Atoms are the same = non polar
  • 2 atoms are different = polar
30
Q

Shape of AX2 and polarity

A
  • Linear
  • Peripheral atoms are same = non polar
  • Peripheral atoms are different = polar
31
Q

Shape of AX2E2 and polarity

A
  • V- shaped

- Central atom has lone pairs = polar

32
Q

Shape of AX3E and polarity

A
  • Trigonal Pyramidal

- Central atom has lone pairs= polar

33
Q

Shape of AX4 and polarity

A
  • Tetrahedral
  • Peripheral atoms are same = non polar
  • Peripheral atoms are different = polar
34
Q

Shape of AX3 and polarity

A
  • Trigonal Planar
  • Peripheral atoms are same = non polar
  • Peripheral atoms are different = polar

Chemistry (6 decks)

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