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Chemistry > The Chemical Bond > Flashcards

The Chemical Bond Flashcards

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1
Q

What is a polyatomic ions?

A

Covalent bonded set of 2 or more atoms that can be considered to behave as a single unit & that has a net charge that is not zero

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2
Q

Formula for ammonium

A

NH4+

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3
Q

Formula for hydroxide

A

OH-

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4
Q

Formula for Chlorate

A

ClO3-

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5
Q

Formula for nitrate

A

NO3-

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6
Q

Formula for carbonate

A

CO3 2-

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7
Q

Formula for chromate

A

CrO4 2-

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8
Q

Formula for sulphate

A

SO4 2-

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9
Q

Formula for phosphate

A

PO4 3-

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10
Q

Formula for cyanide

A

CN-

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11
Q

Formula for acetate

A

C2H3O2-

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12
Q

What a intramolecular bonds?

A

Bonds between atoms forming compounds

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13
Q

What are the 3 types of intermolecular bonds?

A

Ionic bonds
Covalent bonds
Metallic bonds

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14
Q

Strength of the different types of intramolecular bonds (typically)

A

Ionic > metallic > covalent

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15
Q

What is the weakest kind of intramolecular bonds

A

Covalent

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16
Q

What is the strongest kind of intramolecular bonds

A

Ionic

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17
Q

What is the difference between intramolecular bonds & intermolecular forces?

A

intramolecular bonds form molecules, intermolecular forces is the attraction between molecules/atoms

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18
Q

Definition of intermolecular forces

A

Attraction between molecules/atoms to other molecules/atoms

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19
Q

What or the 3 types of intermolecular forces?

A

London dispersion forces
Dipole-dipole interactions
Hydrogen bonds

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20
Q

Are intramolecular bonds week or strong?

A

Strong

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21
Q

Are intermolecular forces strong or weak?

A

Weak

22
Q

Strength of the different types of intermolecular forces (typically)

A

Hydrogen bond > dipole-dipole > London dispersion

23
Q

What is an ionic bond?

A

Where an electron is taken by an electronegative non-metal from an electropositive metal

24
Q

When do ionic bonds occur?

A

When the electronegativity difference between 2 elements is >2

25
Q

What is a metallic bond?

A

Electrons shared between metal atoms

26
Q

What does metallic bonds form?

A

An electron Sea: valence electrons are delocalized & move freely among the metals

27
Q

What is a covalent bond?

A

Where an electron is shared between 2 atoms resulting in a molecule

28
Q

How are molecules made?

A

Covalent bonds

29
Q

How are charged particles made?

A

Ionic bonds

30
Q

What a the 2 kinds of covalent bonds

A

Non-polar covalent & polar covalent

31
Q

When are molecules non-polar?

A

When charge is evenly distributed

32
Q

When are molecules polar?

A

When one the atoms in the molecule have difference in electronegativity making the charge not evenly distributed

33
Q

What molecules are non-polar?

A

Single element molecules: 02, N….
Carbon hydrogen only molecules:CH4, C3H8…
Symmetrical molecules:CCl4, CO2…
Electrongativity difference is very low, <0.5

34
Q

What molecules are polar?

A

Non- symmetrical molecules:CH3Cl, H2O….
Molecules w/ different elements that don’t cancel out

35
Q

How many electrons are shared in a single, double & triple bond?

A

Single: 2
Double: 4
Triple: 6

36
Q

What is bond strength?

A

Energy required to break the bonds

37
Q

Bond strength

A

Triple > double > single

38
Q

Length of bonds, single, double & triple

A

single > double > triple

39
Q

What is bond length?

A

Distance between the nuclei in participating atoms

40
Q

What increases bond length?

A

The number of bonds (the less the longer)
Atomic radius (the bigger the radius the longer)

41
Q

How are bond length & strength related?

A

As bond length increases, strength decreases

42
Q

What kind of bonds does single bonds have?

A

1 sigma bond

43
Q

What kind of bonds does double bonds have?

A

1 sigma bond
1 pi bond

44
Q

What kind of bonds does triple bonds have?

A

1 sigma bond
2 pi bond

45
Q

What are some octet exceptions when making Lewis structures?

A

Period 3 elements occasionally form more than 4 bonds
Sometimes an incomplete octet will form

46
Q

What is the formula for finding lone pairs on central atom? & when does it not work?

A

Lp = (ve - 8n)/2
Lp = lone pairs on central atom
Ve = valence electrons in the entire molecule
N = number of atoms attached to central atom

Does not work with molecules with hydrogen!

47
Q

What is important to remember when drawing vsepr diagrams?

A

Bonds want to be as for away from eachother as possible
Lone pairs cause additional repulsion

48
Q

What are electron domains?

A

Bonding: single, double or triple bonds
Non bonding: lone pairs

49
Q

How many electron domains is a single bond?

A

1

50
Q

When are hydrogen bonds the strongest?

A

When hydrogen is bonded to F, O or N

51
Q

Compounds containing only Carbon & hydrogen are always polar or non polar?

A

Non polar

52
Q

Which are the only inter molecular forces present in Carbon, hydrogen only compounds?

A

London dispersion forces (van der Waals )

Chemistry (10 decks)

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