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CHEM-1315 > Unit 4.4: Explain Covalent Bonds in Molecules and Identify Characteristics of Covalent Bonds > Flashcards

Unit 4.4: Explain Covalent Bonds in Molecules and Identify Characteristics of Covalent Bonds Flashcards

1
Q

Reading 6.2: Covalent Bonding

Hydrogen forms only one bond in covalent bonds, fillings its 1s valence shell

A

Duet rule

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2
Q

Reading 6.2: Covalent Bonding

Atoms gain, lose, or share electrons to achieve a noble gas configuration, ns2 np6 (eight electrons).

A

Octet rule

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3
Q

Reading 6.2: Covalent Bonding

How many bonds is a carbon atom likely to make in a molecule?

A

4

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4
Q

Reading 6.2: Covalent Bonding

How many bonds is a nitrogen atom likely to make in a molecule?

A

3

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5
Q

Reading 6.2: Covalent Bonding

How many bonds is an oxygen atoms likely to make in a molecule?

A

2

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6
Q

Reading 6.2: Covalent Bonding

How many bonds is a flourine atom likely to make in a molecule?

A

1

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7
Q

Reading 6.2: Covalent Bonding

How many bonds is a neon atom likely to make in a molecule?

A

None

Neon already satisfies the octet rule.

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8
Q

Reading 6.2: Covalent Bonding

Diagram of a molecule or polyatomic ion showing shared pairs or bonds as straight lines and unshared or lone pairs as dots

A

Lewis Structure

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9
Q

Reading 6.2: Covalent Bonding

Unshared pairs of electrons in molecules or polyatomic ions.

A

Lone pairs

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10
Q

Reading 6.2: Covalent Bonding

A bond consisting of two atoms, sharing one pair of electrons as shown as a short, straight line in the Lewis structures

A

Single bond

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11
Q

Reading 6.2: Covalent Bonding

A bond consisting of two atoms sharing two pairs of electrons as shown as two short lines in Lewis structures

A

Double bond

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12
Q

Reading 6.2: Covalent Bonding

A bond consisting of two atoms sharing three pairs of electrons and shown as three short lines in Lewis structures

A

triple bonds

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13
Q

Reading 10.9: Bond Enthalpy

The enthalpy change, associated with breaking a specific bond in 1 mol of gaseous molecules.

A

Bond Enthalpies

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14
Q

Reading 10.9: Bond Enthalpy

Energy must be (added/released) to break bonds

A

added

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15
Q

Reading 10.9: Bond Enthalpy

Breaking bonds is (exothermic/endothermic)

A

endothermic

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16
Q

Reading 10.9: Bond Enthalpy

Energy is (added/released) when bonds are formed

A

Released

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17
Q

Reading 10.9: Bond Enthalpy

Bond making is (exothermic/endothermic)

A

exothermic

18
Q

Reading 10.9: Bond Enthalpy

As bond length increases, bond enthalpy (increases/decreases).

A

Decreases

19
Q

Reading 10.9: Bond Enthalpy

Longer bonds tend to be (weaker/stronger) than shorter bonds

A

Weaker

20
Q

4.4 Lecture notes

What holds moelcules together in covalent bonds?

A

Attracting nuclei of both atoms

21
Q

4.4 Lecture notes

What are the three electrostatic interactions in covalent bonds?

A
  1. Attractions between electrons and nuclei
  2. Repulsions between electrons
  3. Repulsions between nuclei
22
Q

4.4 Lecture notes

Attractive forces must _ the repulsive forces for covalent molecules

A

Exceed

23
Q

4.4 Lecture notes

Valence bond theory

A

Atomic orbitals overlap to share electrons

24
Q

4.4 Lecture notes

If atoms get too close, then the 2 nuclei (attract/repulse) each other, and the interaction energy (increases/decreases)

A
  1. Repulse
  2. Increases
25
Q

4.4 Lecture notes

As the distance between the two nuclei decreases, electrons can form a bond by _ their atomic orbitals

A

Overlapping

26
Q

4.4 Lecture notes

The energy needed to overcome the attraction between the nuclei and the shared electrons.

A

Bond Energy

27
Q

4.4 Lecture notes

The number of electron pairs being shared by a given pair of atoms

A

Bond Order

28
Q

4.4 Lecture notes

What two factors do bond lengths depend on?

A
  1. The size of the atom
  2. the strenght of the electronegative differences
29
Q

4.4 Lecture notes

Bonds get (stronger/weaker) and (longer/shorter) down a group.

A
  1. weaker
  2. longer
30
Q

4.4 Lecture notes

Bonds get (weaker/stronger) across a perod.

A

Stronger

31
Q

4.4 Lecture notes

The more electrons two atoms share, the (weaker/stronger) and (longer/shorter) the bonds get.

A
  1. Stronger
  2. Shorter
32
Q

4.4 Lecture notes

What states can molecular compounds exist in?

A
  1. Solid
  2. Liquid
  3. Gas
33
Q

4.4 Lecture notes

Intermolecular forces: IMFs

A

hydrogen bonds

34
Q

4.4 Lecture notes

Which is stronger?
1. IMFs
2. Covalent bonds

A

Covalent bonds

35
Q

4.4 Lecture notes

Which bonds are broken in the gas phase?

A

IMFs

36
Q

4.4 Lecture notes

The hardness and britleness of molecular compounds should vary depinging on what?

A

The strength of intermolecular attractive forces

37
Q

4.4 Lecture notes

Molecular compounds have (high/low) melting and boiling points.

A

Low

38
Q

4.4 Lecture notes

What degree are molecular compounds melting points generally lower than?

A

< 300 degrees celcius

39
Q

4.4 Lecture notes

Do all covalent compounds conduct electricity?

A

No

40
Q

4.4 Lecture notes

Which kind of covalent compounds do conduct electricity?

A

Acids

41
Q

4.4 Lecture notes

What state do acids have to be in to conduct electricity?

A

dissolved in water

CHEM-1315 (27 decks)

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