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Chemistry 90% > Atoms & molecules > Flashcards

Atoms & molecules Flashcards

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1
Q

Atomic number (Z)

A

no of protons (no of electrons)

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2
Q

Atomic mass (A)

A

no of protons and neutrons

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3
Q

Atomic orbital

A

The regions of space surrounding the nucleus where there is high possibilities of finding an electrons

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4
Q

Molecular orbital

A

The region of space surrounding the molecules’ nucleus where may or may find an electrons

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5
Q

Covalent Bond

A

Non- metal & non- metal sharing electrons to fill the outer shell

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6
Q

Ionic Bond

A

Non- metal & metal gain or lose electrons to fill their outer shell

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7
Q

Metallic Bond

A

Bond between metal and metal; lattice structure; seas of electrons; Outer electrons delocalised

Good conduction of electrical when it’s solid but not when it’s liquid as the lattice structure no longer exists

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8
Q

Carbon - Carbon bond

A
  • Single carbon bond (1 sigma)
  • Double carbon bond (1 sigma, 1 pi)
  • Triple carbon bond (1 sigma, 2 pi)
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9
Q

Matter

A

Anything that has a mass and take up space

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10
Q

Substance

A

single, pure form of matter

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11
Q

States of matter

A

Gas, Liquid, Solid

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12
Q

Mixture and Compounds

A

Mixtures

  • Components can be separated by physical method
  • Composition is variable
  • properties are related to its component

Compounds

  • Components cannot be separated by physical method
  • Composition is fixed
  • properties are unlike to its component
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13
Q

Physical properties

A

Characteristics we can observe without changing the identity of the substance e.g. colour, temperature, states of matter, density, hardness

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14
Q

Chemical properties

A

ability of substance change into another substance

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15
Q

Isotopes

A

Same element with different atomic mass: having same number of protons and electrons but different number of neutrons

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16
Q

Protons give the atom _________

A

Identity

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17
Q

Electrons give the atom

A

personality

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18
Q

Atomic radius

A

the distance between the nucleus to the valence electrons

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19
Q

Total number of electrons at different sub shells

A

1st shell - 2
2nd shell - 8
3rd shell - 18
4th shell - 32

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20
Q

No of electrons at different orbitals

A

s- 2
p - 6
d - 10
f - 14

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21
Q

Each orbitals has how many electrons?

A

2

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22
Q

The 2 electrons in the same orbital has ______spin

A

opposite spin

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23
Q

Hierarchy of sub shells

A

1s >
2s> 2p >
3s > 3p > 4s> 3d > 4p >5s

24
Q

Periodic table:
Groups
Blocks
Period

A

Periods: Down the periodic table; Similar properties; valence sub shells
Blocks - last orbital to be filled
Groups - across the periodic table; trend in properties; valence e-

25
Q

Atomic radius _______ across the period because ?

Attraction between nucleus and outer electrons __________

A
  • Decreased
  • Nucleus charge increase; Valence e- added onto the same shell
  • Increased
26
Q

Atomic radius _______ down the groups because ?

Attraction between nucleus and outer electrons __________

A
  • Increased
  • More no of sub shells added, valence e- is further from the nucleus with greater shielding
  • Decreased
27
Q

Group 1 has (how many) valence e-
Group 2 has (how many) valence e-
Group 7 has (how many) valence e-

A

Group 1 - 1 e-
Group 2 - 2 e-
Group 7 - 5 e- (because they have a p valence orbital) (They have 7 outer shell e- , 1 short from the electronic configuration of noble gas)

28
Q

For Group 1 & 2 elements, reactivity ________ down each group
For Group 7, reactivity ________ down each group

A
  • Increase

- Decrease

29
Q

Noble gas

A

Full filled outer shell, s2 p6 electronic configuration

Non reactive

30
Q

Electro- negativity

A

Measure of attraction of an atom for the shared e- in the chemical bond. It is related to the ionisation energy

31
Q

Group 1 & 2 elements are strong _______ agents, they tend to ______
Group 7 elements are strong _______ agents, they tend to ________

A
  • reducing agents/ oxidise

- oxidising agents/ reduce

32
Q

Transition metal

A
  • d block element
  • Metal/ good electricity conductors because of their lattice structure and the sea of e- / Mostly hard, shiny, solid
  • Mercury is an exceptional example
33
Q

Dative bond /Co-ordinate bond

A

e- pairs donors

34
Q

Octet Rule

A

Atoms try to fill its valence shell/ achieve the s2 p6 electronic configuration to become stable

35
Q

Intramolecular Force (Interactive bond)

A
  • Bonding between molecules: ionic/ metallic/ covalent

- Affects chemical properties

36
Q

Intermolecular force (Attractive bond)

A
  • Bonding within the molecule: hydrogen/ permanent Dipole Dipole interactions/ Van de Waal’s force
  • Affects physical properties
37
Q

Which elements are most likely to form hydrogen bonding

A

H (delta +) - O/ F/ N (delta -)

38
Q

ionisation energy

A

Ability (Energy needed) for the atom to lost its electrons

39
Q

Hybridisation

A
  • Overlap of two different energy level of orbitals

- Has the properties of the mixed orbitals

40
Q

No of orbits at each sub level (s, p, d, f)

A

s- 1 / p- 3 / d- 5 / f- 7

41
Q

valency

A

no of e- in the valence shell

42
Q

cation

A

+ve ions; tend to be metals

43
Q

anion

A
  • ve ions; tends to be non-metals
44
Q

2 p^6

where to find the element in the periodic table?

A

2- period
p - block
6 - group within block

45
Q

polyatomic ion

A

ion with different element

46
Q

homonuclear combination

A

atoms of the same element

47
Q

What is sigma bond

A

overlap of two orbitals - head to head > s- s / s - p

Overlap of two s orbitals > s- s

48
Q

What is pi bond

A

over lap of p orbitals - side to side > p - p

49
Q

dipole

A

uneven distribution of e-

50
Q

pi bond has more energy than sigma bond. why?

A

the overlap of orbitals

p orbital e- has more energy than s orbital e-

51
Q

same repel, opposite attract

A

True

52
Q

Like dissolve like

A

True

53
Q

If a pair of shared e- is pulled closer to one of the atom. Describe it

A

Unevenly shared e- = unequal distribution of negative e- charge (e- density)

54
Q

Triple covalent bond is more reactive and stronger than single bond T/F

A

False

Triple bond is more reactive and has more energy as in higher e- density BUT NOT stronger

55
Q

Electronegativity range of values

A

0 - 0.4 > non- polar covalent (no dipole)
0.4- 1.7 > polar covalent (Dipole) (more polar / less polar)
> 1.7 - ionic

Chemistry 90% (7 decks)

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