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Chemistry > Module 2.2 > Flashcards

Module 2.2 Flashcards

1
Q

Define an orbital:

A

A region of space 2 electrons can occupy, region with the highest probability of electrons being there.

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2
Q

What shape are S orbitals?

A

Spherical

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3
Q

What shape are P orbitals?

A

8 shape

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4
Q

Define isoelectric:

A

Same electron config as a different element

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5
Q

Define ‘ground state’:

A

All the electrons are in the lowest energy level.

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6
Q

Define ‘excited’:

A

Electrons in a higher that expected energy lever, further out shell.

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7
Q

Describe afbaus theory:

A

Electrons occupy lowest possible energy levels, want to be in ground state.

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8
Q

Describe Hunds rule of multiplicity:

A

Electrons will only occupy an occupied orbital if there are no others, still following law of filling.
Electrons sharing orbitals will have an opposite spin.

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9
Q

Which to elements don’t follow the pattern of the periodic table electron configuration?

A

Chromium and copper

Cr 4s1 3d5
Cu 4s1 3d10

Because they are more stable.

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10
Q

Why don’t transition metals follow the periodic table electron config pattern?

A

When positive ions are formed, 4s electrons are lost first.

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11
Q

Define covalent bond:

A

Electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms.
Non metals bonded to non metals.

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12
Q

Define ionic bonding:

A

Electrostatic attraction between oppositely charged ions.

Metals bonded to non metals

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13
Q

Name for a metal ion?

A

Cation

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14
Q

Name for a non metal ion

A

Anion

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15
Q

Define a metallic bond:

A

Electrostatic attraction between positively charged metal ions and delocalised electrons.

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16
Q

What happens as the charge of an ion increases in a metallic bond?

A

More electrons lost, stronger the metallic bond.

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17
Q

How many electrons can an orbital hold?

A

2

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18
Q

What kind of electron configuration do elements want to achieve by bonding?

A

That of the noble gases

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19
Q

What are dative covalent bonds sometimes called?

A

Coordinate bonds

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20
Q

Describe a dative covalent bond:

A

Covalent bond where both electrons come from same atom.

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21
Q

Describe simple covalent molecules:

A

Small molecules
Don’t conduct electricity
No ions or free electrons
Soluble in organic compounds, not water

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22
Q

Describe the structure of diamond:

A

Carbon covalent ly bonded to 4 others

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23
Q

Describe the properties of diamond:

A

High melting point
Doesn’t conduct electricity, no ions or delocalised electrons
V hard
Insoluble

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24
Q

Describe the structure of graphite:

A

Carbon covalently bonded to 3 others

Delocalised electrons between layers

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25
Q

Ion of aluminium

A

Al3+

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26
Q

Ion of ammonium

A

NH4+

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27
Q

Ion of barium

A

Ba2+

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28
Q

Calcium ion

A

Ca2+

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29
Q

Copper 2 ion

A

Cu2+

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30
Q

Lead ion

A

Pb2+

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31
Q

Silver ion

A

Ag+

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32
Q

Zinc ion

A

Zn2+

33
Q

Carbonate ion

A

CO3 2-

34
Q

Hydrogen carbonate ion

A

HCO3 -

35
Q

Hydroxide ion

A

OH-

36
Q

Nitrate ion

A

NO3 -

37
Q

Sulfate ion

A

SO4 2-

38
Q

Define electonegativity:

A

The ability for an element to attract the electron pair in a covalent bond to itself

39
Q

Describe a non-polar bond:

A

Same electronegativity
Electrons shared
100% covalent

40
Q

Describe a polar bond:

A

One pulls electrons closer to its end one is slightly more positive, one is more negative

41
Q

Describe the Pauling scale

A

Measures electonegativity
N O F Cl Br
>0.4 difference gives polarity

42
Q

Define a dipole

A

An uneven distribution of electrons

43
Q

What is the strongest type of intermolecular bond?

A

Hydrogen bonding

Mainly in water

44
Q

What does a hydrogen bond need?

A

H atom attached to an electronegative oxygen fluorine of nitrogen
O F N must have a lone pair of electrons

45
Q

Boiling point of water and methane

A

100* C

-164* C

46
Q

Where is the H bond in water?

A

From the lone pair of oxygen electrons to the electron deficient hydrogen ion

47
Q

3 types of dipole:

A

Permanent
Induced
Instantaneous

48
Q

Describe a permenant dipole:

A

Uneven distribution of electrons

One element in molecule is more electronegative so pulls the electrons to one side

49
Q

Describe an induced dipole:

A

E.g. Cl-Cl H-Cl
The HCl causes the chlorine to have a dipole.
Electrons pulled away from Cl on left to Cl on right np y electron deficient hydrogen

50
Q

Describe an instantaneous dipole:

A

Between elements with same electronegativity
Electrons not equally dispersed around atom, maybe one side
Electrons randomly move towards one atom
No cause
May cause an induced dipole in neighbouring molecules
More shells=more electrons=larger risk of instantaneous

51
Q

Valence definition

A

Outer shell

52
Q

2bp

A

180* linear

53
Q

3pb

A

120* trigonal planar

54
Q

4bp

A

109.5 tetrahedral

55
Q

5bp

A

120*
90*
Trigonal by pyramid

56
Q

6bp

A

90*

Octahedral

57
Q

3bp 1lp

A

107*

Pyramidal

58
Q

How much do lone pairs reduce bond angles by?

A

2.5

59
Q

2bp 2lp

A

Non linear

104.5

60
Q

Example of a linear molecule

A

Carbon dioxide

61
Q

Example of a trigonal planar molecule

A

Boron triflouride

62
Q

Example of a tetrahedral molecule

A

Methane

63
Q

Boron trifluoride formula

A

BF3

64
Q

Methane formula

A

CH4

65
Q

Trigonal by pyrimadol molecule example

A

Phosphorus pentachloride

66
Q

Phosphorus pentachloride formula

A

Pcl5

67
Q

Octahedral molecule example

A

Sulfur hexaflouride

68
Q

Soulful hexaflouride formula

A

SF6

69
Q

Pyramidal molecule example

A

Ammonia

70
Q

Ammonia formula

A

NH3

71
Q

Non linear molecule example

A

Water

72
Q

3 types of van der waals forces

A

Permanent dipole - permanent dipole attraction
Permanent dipole - induced dipole attraction
Instantaneous dipole - induced dipole attraction

73
Q

What are the 4 types of crystalline structure?

A

Giant ionic structure
Simple molecular structure
Macromolecular structure
Metallic structure

74
Q

Acid + Base =

A

Salt + water

75
Q

Metal oxide + Acid =

A

Salt + water

76
Q

Metal hydroxide + Acid =

A

Salt + Water

77
Q

Metal + Acid =

A

Metal Salt + Hydrogen

78
Q

Metal carbonate + acid =

A

Metal salt + carbon dioxide + water

Chemistry (7 decks)

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