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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
Describe triple bond
Strong bond between two atoms formed by three pairs of electrons that are shared by the two nuclei
26
State the greek prefix of 1
mono-
27
State the greek prefix of 5
penta-
28
State the greek prefix of 6
hexa-
29
State the greek prefix of 7
hepta-
30
State the greek prefix of 8
octa-
31
State the greek prefix of 9
nona-
32
State the greek prefix of 10
deca-
33
Describe non-polar covalent bonds
Covalent bonds in which the bonding electron pairs are shared equally between the nuclei of two bonded atoms
34
Describe polar covalent bonds
Covalent bonds in which the bonding electrons are unequally shared between the nuclei of two bonded atoms
35
Describe binary molecular compounds
Compounds composed of two elements
36
Describe bond dipole
Separation of charge in a polar covalent bond
37
State whether or not a polar covalent bond is purely covalent
No. There are some characteristics of ionic bonding held by the molecule.
38
Describe non-polar molecules
Molecules containing only non-polar bonds or polar bonds which are cancelled out by molecular structure
39
Describe polar molecules
Molecules where one end of the molecules is slightly positive and the other slightly negative
40
Provide an alternative term to polar molecule
Dipole molecule
41
State what all polar molecules are composed of
Polar bonds
42
State whether or not all molecule with polar bonds are polar
No. Some molecules with polar bonds are non-polar
43
State what the polarity of a molecules is dependent upon
The direction of the bond dipoles in a molecule
44
Describe intramolecular bonding
Involving the internal structure of a molecule
45
Describe intermolecular bonding
Involving the external structure/interaction of molecules
46
State the 2 types of bonding
- intermolecular | - intramolecular
47
Compare and contrast intermolecular and intramolecular bonding
Intramolecular bonds reference the bonds within molecules, whereas intermolecular bonds refer to the attractive or repulsive forces between molecules
48
State whether or not covalent bonding is an intramolecular or intermolecular bond
Intramolecular bond
49
State whether or not ionic bonding is an intramolecular or intermolecular bond
Intramolecular bond
50
State whether or not metallic bonding is an intramolecular or intermolecular bond
Intramolecular bond
51
State the 2 factors which influence the strength of dispersion forces
1. number of electrons in molecules | 2. molecular shape (how close molecules approach each other)
52
State what increases as the proximity between two molecules increases
Strength of intermolecular forces
53
State the weakest of the intermolecular forces
Dispersion forces
54
State whether or not dispersion forces can occur between instantaneous dipoles
Yes. Dispersion forces can occur between instantaneous dipoles.
55
State the strongest of the intermolecular forces
Hydrogen bonding
56
State what molecules dipole-dipole interactions can occur between
Polar molecules
57
Describe dispersion forces
Bond between adjacent molecules formed by instantaneous dipoles
58
Describe hydrogen bonding
Bond between a hydrogen atom covalently bonded to an atom of F, O, N
59
Describe dipole-dipole forces
Weak bonding caused by the positive end of one dipole attracting the negative end of another dipole
60
State between what elements a hydrogen bond can form
H and N, O, F
61
Describe the effects of hydrogen bonding on the properties of water
- high melting/boiling points | - expansion of water upon freeing
62
State what occurs when the electrons of hydrogen move slightly towards the bonding element during hydrogen bonding
The H nucleus becomes unshielded and a dipole forms
63
Describe instantaneous dipoles. State how they occur.
Dipoles that exist for only an instant and for which formation is random. Occur due to random movement of electrons within the molecule.
64
Describe induced dipoles. State how they occur.
Weak attraction that results when a polar molecule disturbs the arrangement of electrons in a non-polar species
65
State the 5 molecular shapes
1. tetrahedral 2. pyramidal 3. V-shaped 4. linear 5. planar
66
Describe the molecular shape of a compound with 4 bonding pairs around a central atom
Tetrahedral
67
Describe the molecular shape of a compound with 3 bonding pairs around a central atom
Pyramidal
68
Describe the molecular shape of a compound with 2 bonding pairs around a central atom
V-shaped
69
Describe the molecular shape of a compound with 2 bonding pairs for each central atom
Linear
70
Describe the molecular shape of a compound with 3 bonding pairs for each central atom
Planar
71
State what the physical properties of a compound are dependent upon
Type of bonding it displays
72
State whether or not molecular substances conduct electricity in the solid or molten form
Molecules do not conduct electricity because the molecules are electrically neutral
73
State whether or not molecular substances conduct electricity if dissolved in water
Molecules do not conduct electricity because the molecules are electrically neutral
74
State whether or not molecular substances vary in their solubility in water and other solvents
Yes. Solubility varies
75
State whether or not molecules that dissolve in water and produce ions can conduct electricity
Yes. Owing to the movement of ions, electricity can be conducted
76
State whether or not polar compounds are soluble in polar solvents
Yes.
77
State whether or not polar compounds are soluble in non-polar solvents
No.
78
State whether or not non-polar compounds are soluble in non-polar solvents
Yes.
79
State whether or not non-polar compounds are soluble in polar solvents
No.
80
Provide the rule that outlines solubility of compounds
'like dissolves like'
81
Describe the common state of molecular substances at room temperature
Gas/liquid
82
Describe the malleability of molecular substances
Mostly soft and easily scratched
83
Define molecular substances
Substance that consists of two or more atoms that is joined together by a covalent bond.
84
List the 3 major types of molecular models used to represent molecules
1. ball and stick 2. space filling 3. computer generated
85
Describe the limitations of electron dot diagrams and structural formula in representing the shapes of molecules
Do not show the three dimensional shapes of molecules
86
Describe dipole
Structure with two oppositely charged areas
87
Provide the molecular formula of two covalently bonded chlorine atoms
Cl2
88
Provide the structural formula of two covalently bonded chlorine atoms
Cl-Cl
89
State the greek prefix of 2
-di
90
State the greek prefix of 3
-tri
91
State the greek prefix of 4
-tetra

C11 (13 decks)

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