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Chemistry 20 > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

1
Q

What is an orbital?

A

Region of space around an atoms nucleus where an electron may exist

It’s a 3D space that defines where an electron may be

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2
Q

What are the four rules of Bonding Theory?

A

The first energy level has room for only one orbital = 2 electron math

Energy levels above the first have room for four orbitals = 8 electrons max

An orbital can be unoccupied or it may contain one or two electrons - but never more then two

Electrons spread out to occupy any empty valence orbitals before forming electron pairs

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3
Q

What are Lewis Symbols?

A

Named after Gilbert Lewis who is responsible for the Octet Rule. He reasoned that all atoms strive to be like the nearest noble gas

Used dots or x to represent the valence electrons

The inner electrons and the nucleus are represent by the element symbol

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4
Q

What is electronegativity?

A

A measure of the force that an atom exerts on electrons of other atoms

The greater number the greater the force

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5
Q

How do we assign each atom an electronegativity?

A

The greater number of protons in the nucleus, the greater the attraction for more electrons

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6
Q

What is covalent bonding?

A

Both atoms have a high EN so neither atom “wins”

The EN difference can be zero or small

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7
Q

What is ionic bonding?

A

The electronegativity of the two atoms are quite different

The atom with the higher EN will remove the bonding electron from the other atom (electron transfer occurs)

Positive and negative ions are formed which attract each other

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8
Q

What is metallic bonding?

A

Both atoms have a relatively low EN so atoms share valence electrons, but no actual chemical reaction takes place

Electrons are not held very strongly by their atoms

The atoms have vacant valence orbitals

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9
Q

What is VSEPR?

A

Valence Shell Electron Pair Repulsion

Pairs of electrons remain as far apart as possible due to the repulsive forces of their negative energy

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10
Q

What is the VSEPR shape linear?

A

Two bonds and no lone pairs on the central atom

Bond angle: 180

General form: AX2

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11
Q

What is the VSEPR shape trigonal planar?

A

Three bonds and no lone pairs on the central atom

Bond angle: 120

General form: AX3

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12
Q

What is the VSEPR shape tetrahedral?

A

Four bond and no lone pairs on the central atom

Bond angle: 109.5

General form: AX4

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13
Q

What is the VSEPR shape trigonal pyramidal?

A

Three bonds and one lone pair on the central atom

Bond angle: 107.3

General form: AX3E

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14
Q

What is the VSEPR shape angular?

A

Two bonds and two lone pairs on the central atom

Bond angle: 105

General form: AX2E2

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15
Q

What is the VSEPR shape linear (tetrahedral)?

A

Two bonds and three lone pairs on the central atom

Bond angle: 109.5

General form: AXE3

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16
Q

What is polarity?

A

Partial positive and negative charges on opposite sides of the molecule

A molecule with symmetrical electron distribution is a non polar molecule

17
Q

What does “Like Dissolves Like” mean?

A

Polar substances are soluble in polar substances, non polar substances are soluble in non polar substances

18
Q

What is Bond Energy?

A

The energy required to break a chemical bond or the energy released when a bond is formed

19
Q

What are the three types of forces in matter?

A

Intranuclear force

Intramolecular force

Intermolecular force

20
Q

What is intranuclear force?

A

Bonds within the nucleus between protons and neutrons (very strong)

21
Q

What is intramolecular force?

A

Bonds between atoms within the molecule or between ions within the crystal lattice (quite strong)

22
Q

What is intermolecular force?

A

Bonds between molecules (quite weak) and are electrostatic (involve positive and negative charges)

23
Q

What are the three types of intermolecular bonds?

A 
London Force (weakest)
Dipole-Dipole Force (medium)
Hydrogen Bonding (strongest)
24
Q

What is London Force?

A

Momentary forces of attraction between molecules

Created as electrons circulate to make momentary weak dipoles

All molecular compounds have LDF

The more electrons in a molecule means greater LDF

25
Q

What are Dipole-Dipole Bonds?

A

Permanent attractive forces between polar molecules

The molecules line up positive end to negative end

The greater the overall polarity in a molecule, the greater the strength of the dipole interaction

26
Q

What are Hydrogen Bonds?

A

Strongest intermolecular force

Exists only for molecules with an H atom bonded to a N, O, or F atom

Chemistry 20 (2 decks)

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