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C11 > Covalent Bonding > Flashcards

Covalent Bonding Flashcards

1
Q

Describe covalent bond

A

Bonds are formed when atoms share electrons

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2
Q

Compare and contrast ionic bonds with covalent bonds

A

Ionic bonds require a transfer of electrons and covalent bonds do not

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3
Q

Describe the trend in the boiling and melting points of non-metals

A

Low melting and boiling points

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4
Q

Describe the ability of non-metals to conduct electricity

A

Poor conductors

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5
Q

Outline the inference that can be drawn about the force of attraction between non-metals based on their boiling and melting points

A

They have low boiling and melting points making the forces of attraction between particles very weak

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6
Q

Outline the inference that can be drawn about the movement of charged particles through the substance based on the ability of non-metals to conduct electricity

A

They are poor conductors meaning that no charged particles are free to move through the substance

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7
Q

State what the basic units of covalent molecular substance are

A

Molecules

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8
Q

State which atoms within a molecule share electrons

A

Adjacent atoms

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9
Q

State what the electrical attraction between the nuclei of adjacent atoms and the shared electrons is referred to as

A

Covalent bonding

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10
Q

State what the overall charge of each molecule held together by covalent bonds is

A

Zero

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11
Q

State how adjacent molecules are held together if covalently bonded molecules have a net charge of zero

A

Intermolecular forces

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12
Q

Describe a covalent molecular element

A

Atoms of identical elements share electrons with each other

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13
Q

Describe diatomic molecules

A

Substance containing only two atoms

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14
Q

Describe discrete molecules

A

Separated and distinct from surrounding molecules

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15
Q

Provide an example of elements that exist as discrete atoms

A

Noble gases

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16
Q

Provide an example of a diatomic molecule

A

H2

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17
Q

Describe a covalent molecular compound

A

Atoms of different elements share electrons with each other

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18
Q

State a term used to refer to atoms with full outer shells

A

Stable

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19
Q

Propose a reason why atoms might share electrons

A

To achieve a full outer shell

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20
Q

State what electronegativity non-metals usually have

A

High electronegativities

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21
Q

State what the electronegiativity of non-metals assists with

A

Attraction of electrons

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22
Q

State a term used to refer to non-bonding electrons

A

Lone pairs

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23
Q

Describe single bond

A

Bond formed between one pair of electrons shared between two atoms

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24
Q

Describe double bond

A

Strong bond between two atoms formed by two pairs of electrons that are shared by the two nuclei

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25
Q

Describe triple bond

A

Strong bond between two atoms formed by three pairs of electrons that are shared by the two nuclei

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26
Q

State the greek prefix of 1

A

mono-

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27
Q

State the greek prefix of 5

A

penta-

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28
Q

State the greek prefix of 6

A

hexa-

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29
Q

State the greek prefix of 7

A

hepta-

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30
Q

State the greek prefix of 8

A

octa-

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31
Q

State the greek prefix of 9

A

nona-

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32
Q

State the greek prefix of 10

A

deca-

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33
Q

Describe non-polar covalent bonds

A

Covalent bonds in which the bonding electron pairs are shared equally between the nuclei of two bonded atoms

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34
Q

Describe polar covalent bonds

A

Covalent bonds in which the bonding electrons are unequally shared between the nuclei of two bonded atoms

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35
Q

Describe binary molecular compounds

A

Compounds composed of two elements

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36
Q

Describe bond dipole

A

Separation of charge in a polar covalent bond

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37
Q

State whether or not a polar covalent bond is purely covalent

A

No. There are some characteristics of ionic bonding held by the molecule.

38
Q

Describe non-polar molecules

A

Molecules containing only non-polar bonds or polar bonds which are cancelled out by molecular structure

39
Q

Describe polar molecules

A

Molecules where one end of the molecules is slightly positive and the other slightly negative

40
Q

Provide an alternative term to polar molecule

A

Dipole molecule

41
Q

State what all polar molecules are composed of

A

Polar bonds

42
Q

State whether or not all molecule with polar bonds are polar

A

No. Some molecules with polar bonds are non-polar

43
Q

State what the polarity of a molecules is dependent upon

A

The direction of the bond dipoles in a molecule

44
Q

Describe intramolecular bonding

A

Involving the internal structure of a molecule

45
Q

Describe intermolecular bonding

A

Involving the external structure/interaction of molecules

46
Q

State the 2 types of bonding

A
  • intermolecular

- intramolecular

47
Q

Compare and contrast intermolecular and intramolecular bonding

A

Intramolecular bonds reference the bonds within molecules, whereas intermolecular bonds refer to the attractive or repulsive forces between molecules

48
Q

State whether or not covalent bonding is an intramolecular or intermolecular bond

A

Intramolecular bond

49
Q

State whether or not ionic bonding is an intramolecular or intermolecular bond

A

Intramolecular bond

50
Q

State whether or not metallic bonding is an intramolecular or intermolecular bond

A

Intramolecular bond

51
Q

State the 2 factors which influence the strength of dispersion forces

A
  1. number of electrons in molecules

2. molecular shape (how close molecules approach each other)

52
Q

State what increases as the proximity between two molecules increases

A

Strength of intermolecular forces

53
Q

State the weakest of the intermolecular forces

A

Dispersion forces

54
Q

State whether or not dispersion forces can occur between instantaneous dipoles

A

Yes. Dispersion forces can occur between instantaneous dipoles.

55
Q

State the strongest of the intermolecular forces

A

Hydrogen bonding

56
Q

State what molecules dipole-dipole interactions can occur between

A

Polar molecules

57
Q

Describe dispersion forces

A

Bond between adjacent molecules formed by instantaneous dipoles

58
Q

Describe hydrogen bonding

A

Bond between a hydrogen atom covalently bonded to an atom of F, O, N

59
Q

Describe dipole-dipole forces

A

Weak bonding caused by the positive end of one dipole attracting the negative end of another dipole

60
Q

State between what elements a hydrogen bond can form

A

H and N, O, F

61
Q

Describe the effects of hydrogen bonding on the properties of water

A
  • high melting/boiling points

- expansion of water upon freeing

62
Q

State what occurs when the electrons of hydrogen move slightly towards the bonding element during hydrogen bonding

A

The H nucleus becomes unshielded and a dipole forms

63
Q

Describe instantaneous dipoles. State how they occur.

A

Dipoles that exist for only an instant and for which formation is random.
Occur due to random movement of electrons within the molecule.

64
Q

Describe induced dipoles. State how they occur.

A

Weak attraction that results when a polar molecule disturbs the arrangement of electrons in a non-polar species

65
Q

State the 5 molecular shapes

A
  1. tetrahedral
  2. pyramidal
  3. V-shaped
  4. linear
  5. planar
66
Q

Describe the molecular shape of a compound with 4 bonding pairs around a central atom

A

Tetrahedral

67
Q

Describe the molecular shape of a compound with 3 bonding pairs around a central atom

A

Pyramidal

68
Q

Describe the molecular shape of a compound with 2 bonding pairs around a central atom

A

V-shaped

69
Q

Describe the molecular shape of a compound with 2 bonding pairs for each central atom

A

Linear

70
Q

Describe the molecular shape of a compound with 3 bonding pairs for each central atom

A

Planar

71
Q

State what the physical properties of a compound are dependent upon

A

Type of bonding it displays

72
Q

State whether or not molecular substances conduct electricity in the solid or molten form

A

Molecules do not conduct electricity because the molecules are electrically neutral

73
Q

State whether or not molecular substances conduct electricity if dissolved in water

A

Molecules do not conduct electricity because the molecules are electrically neutral

74
Q

State whether or not molecular substances vary in their solubility in water and other solvents

A

Yes. Solubility varies

75
Q

State whether or not molecules that dissolve in water and produce ions can conduct electricity

A

Yes. Owing to the movement of ions, electricity can be conducted

76
Q

State whether or not polar compounds are soluble in polar solvents

A

Yes.

77
Q

State whether or not polar compounds are soluble in non-polar solvents

A

No.

78
Q

State whether or not non-polar compounds are soluble in non-polar solvents

A

Yes.

79
Q

State whether or not non-polar compounds are soluble in polar solvents

A

No.

80
Q

Provide the rule that outlines solubility of compounds

A

‘like dissolves like’

81
Q

Describe the common state of molecular substances at room temperature

A

Gas/liquid

82
Q

Describe the malleability of molecular substances

A

Mostly soft and easily scratched

83
Q

Define molecular substances

A

Substance that consists of two or more atoms that is joined together by a covalent bond.

84
Q

List the 3 major types of molecular models used to represent molecules

A
  1. ball and stick
  2. space filling
  3. computer generated
85
Q

Describe the limitations of electron dot diagrams and structural formula in representing the shapes of molecules

A

Do not show the three dimensional shapes of molecules

86
Q

Describe dipole

A

Structure with two oppositely charged areas

87
Q

Provide the molecular formula of two covalently bonded chlorine atoms

A

Cl2

88
Q

Provide the structural formula of two covalently bonded chlorine atoms

A

Cl-Cl

89
Q

State the greek prefix of 2

A

-di

90
Q

State the greek prefix of 3

A

-tri

91
Q

State the greek prefix of 4

A

-tetra

C11 (13 decks)

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