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Alevel chemistry year2 > Y13 Chem mock > Flashcards

Y13 Chem mock Flashcards

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1
Q

Why are do isotopes have similar chemical properties

A

Same electron configuration which affects the chemical properties of the atoms

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2
Q

Why do isotopes have different physical properties

A

due to the differing masses of the atoms they can have different densities

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3
Q

What did jj thompson add to the understanding of chemistry

A

The atom contains negatively charged particles called electrons, devised the plum pudding model(positive charge with small negative charges dotted)

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4
Q

What did rutherford add to the understanding of chemistry

A

He fired alpha particles at a thin sheet of gold most of the particles went straight through which suggests the atom isn’t entirely positive some of them were reflected. Suggested nuclear model positive nucleus with clouds of electrons that float around it

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5
Q

What modifications did rutherford add

A

Realised that nucleus had positive charge that varied between atoms, determined existence of protons

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6
Q

What did james chadwick discover

A

Existence of neutrons

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7
Q

What is relative atomic mass

A

Ar is the weighted mean mass of an element compared to 1/12 the mass of an atom of C-12

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8
Q

What is the relative isotopic mass

A

Mass of an atom of an isotope compared to 1/12 the mass of c12

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9
Q

What is molar mass

A

The mass of one mole of something (“g mol-1)

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10
Q

What is the gas volume equation

A

number of moles = volume in dm3/24

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11
Q

what is room temp and pressure

A

298k, 100kPa

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12
Q

Ideal gas equation and units

A

pV = nRT
p = Pa kPa to Pa *1000
V= dm3 cm to dm3 /1000 dm3 to m3 /1000
n= moles
R=8.314
T= K *c + 273

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13
Q

concentration equation

A

moles= conc * volume (dm3)

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14
Q

what is the empirical formula

A

smallest number ratio of atoms in a com pound

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15
Q

Important ions

A

Nitrate- No3-
Carbonate- CO32-
SO42-
OH-
NH4+

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16
Q

What are acids, main ones

A

proton donors
HCL
H2SO4
HNO3(nitric)
CH3COOH(ethanoic acid

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17
Q

what are bases, common bases

A

proton acceptors
NaOH
KOH
NH3

18
Q

What is the reaction between ammonia and H20

A

NH3 + H20 -> NH4+ + OH-
reversible

19
Q

Strong bases/ acids

A

HCL fully dissociates in water, and nearly all the H+ ions are released

20
Q

weak bases/ acids

A

backward reaction favoured so small amoutns of acid dissociates in water and few H+ ions are released

21
Q

Acid + Base ->

A

Salt + Water

22
Q

Metal + Acid

A

Salt + Hydrogen

23
Q

Metal oxide + Acid

A

Salt + Water

24
Q

Metal hydroxide + Acid

A

Salt + Water

25
Q

What is the principal quantum number

A

energy levels in which electrons lie(shells)

26
Q

What are subshells

A

Further division of the shells

27
Q

What are orbitals

A

Areas of space in which electrons can be found(cloud) can only hold up to 2 electrons

28
Q

What main property of electron

A

quantum property of spin, they spin in opposite directions they also repel each other to an extent

29
Q

What is a giant ionic lattice

A

repeating regular structure of ironically bonded atoms

30
Q

Behaviours of ionic compounds

A

conductivity in molten/dissolved because ions can move and carry charge
high melting and boiling points ionic compounds are held together by lattice which has strong electrostatic forces
soluability can dissolve in water due to charges hydrogen bonds can form

31
Q

What is a dative bond

A

when an atom donates 2 electrons on its own in a covalent bond

32
Q

What are the special cases for covalent bonds

A

Boron trifluoride (6 electron in outer shell)
Sulphur hexafluoride expands the octet and has 12 electrons in its outer shell

33
Q

What is average bond enthalpy

A

the energy required to break a covalent bond

34
Q

Linear shape

A

2 bonding pairs no lone pairs(180)

35
Q

trigonal planar

A

3 bonding pairs (120)

36
Q

tetrahedral

A

4 bonding pairs(109.5)

37
Q

trigonal pyramidal

A

3 bonding pairs 1 lone pair (107)

38
Q

non-linear

A

2 bonding pairs 2 lone pairs(104.5)

39
Q

trigonal pyramidal

A

5 bonding pairs 120 and 90

40
Q

octahedral

A

6 boning pairs(90)

41
Q
A

Alevel chemistry year2 (2 decks)

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