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Chemistry 90% > Atoms & molecules > Flashcards

Atoms & molecules Flashcards

(55 cards)

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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

Study These Flashcards
A

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

24
Q

Periodic table:
Groups
Blocks
Period

Study These Flashcards
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
Atomic radius _______ across the period because ? | Attraction between nucleus and outer electrons __________
- Decreased - Nucleus charge increase; Valence e- added onto the same shell - Increased
26
Atomic radius _______ down the groups because ? | Attraction between nucleus and outer electrons __________
- Increased - More no of sub shells added, valence e- is further from the nucleus with greater shielding - Decreased
27
Group 1 has (how many) valence e- Group 2 has (how many) valence e- Group 7 has (how many) valence e-
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
For Group 1 & 2 elements, reactivity ________ down each group For Group 7, reactivity ________ down each group
- Increase | - Decrease
29
Noble gas
Full filled outer shell, s2 p6 electronic configuration | Non reactive
30
Electro- negativity
Measure of attraction of an atom for the shared e- in the chemical bond. It is related to the ionisation energy
31
Group 1 & 2 elements are strong _______ agents, they tend to ______ Group 7 elements are strong _______ agents, they tend to ________
- reducing agents/ oxidise | - oxidising agents/ reduce
32
Transition metal
- 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
Dative bond /Co-ordinate bond
e- pairs donors
34
Octet Rule
Atoms try to fill its valence shell/ achieve the s2 p6 electronic configuration to become stable
35
Intramolecular Force (Interactive bond)
- Bonding between molecules: ionic/ metallic/ covalent | - Affects chemical properties
36
Intermolecular force (Attractive bond)
- Bonding within the molecule: hydrogen/ permanent Dipole Dipole interactions/ Van de Waal's force - Affects physical properties
37
Which elements are most likely to form hydrogen bonding
H (delta +) - O/ F/ N (delta -)
38
ionisation energy
Ability (Energy needed) for the atom to lost its electrons
39
Hybridisation
- Overlap of two different energy level of orbitals | - Has the properties of the mixed orbitals
40
No of orbits at each sub level (s, p, d, f)
s- 1 / p- 3 / d- 5 / f- 7
41
valency
no of e- in the valence shell
42
cation
+ve ions; tend to be metals
43
anion
- ve ions; tends to be non-metals
44
2 p^6 | where to find the element in the periodic table?
2- period p - block 6 - group within block
45
polyatomic ion
ion with different element
46
homonuclear combination
atoms of the same element
47
What is sigma bond
overlap of two orbitals - head to head > s- s / s - p Overlap of two s orbitals > s- s
48
What is pi bond
over lap of p orbitals - side to side > p - p
49
dipole
uneven distribution of e-
50
pi bond has more energy than sigma bond. why?
the overlap of orbitals | p orbital e- has more energy than s orbital e-
51
same repel, opposite attract
True
52
Like dissolve like
True
53
If a pair of shared e- is pulled closer to one of the atom. Describe it
Unevenly shared e- = unequal distribution of negative e- charge (e- density)
54
Triple covalent bond is more reactive and stronger than single bond T/F
False | Triple bond is more reactive and has more energy as in higher e- density BUT NOT stronger
55
Electronegativity range of values
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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