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foundations in chemistry Flashcards

1
Q

hydroxide ion

A

OH-

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2
Q

nitrate ion

A

NO3-

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3
Q

ammonium ion

A

NH4+

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4
Q

sulfate ion

A

SO4 2-

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5
Q

carbonate ion

A

CO3 2-

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6
Q

structure of sodium chloride

A

giant ionic structure

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7
Q

why can ionic compounds conduct electricity when molten/ dissolved in solution

A

ions are free to move around

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8
Q

why do ionic compounds have a high mp

A

strong electrostatic forces
between oppositely charged ions
require lots of energy to overcome

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9
Q

what is covalent bonding

A

sharing of outer e- in order for atoms to obtain a full outer shell

electrostatic attraction between shared e- and pos nucleus

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10
Q

what are dative covalent/ coordinate bonds

A

when 1 atom donated 2 e- to an atom or ion to form a bond

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11
Q

eg of dative covalent bonding

A

ammonium

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12
Q

generally what happens to the bond angle when a lone pair is added

A

decreases by 2.5

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13
Q

BeCl2 shape and bond angle

A

2 bond pairs
0 lone pairs
linear
180

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14
Q

BF3 shape and bond angle

A

3 bond pair
0 lone pair
trigonal planar
120

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15
Q

CH4 shape and bond angle

A

4 lone pair
0 bond pair
tetraheldral
109.5

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16
Q

PCl5 shape and bond angle

A

5 bond pairs
0 lone pairs
trigonal bipyrimidal
90
120

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17
Q

SF6 shape and bond angle

A

6 bond pairs
0 lone pairs
octahedral
90

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18
Q

NH3 shape and bond angle

A

3 bond pair
1 lone pair
trigonal pyramidal
107

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19
Q

H20 shape and bond angle

A

2 bond pair
2 lone pair
bent
104.5

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20
Q

ClF3 shape and bond angle

A

3 bond pair
2 lone pair
trigonal planar
120

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21
Q

XeF4 shape and bond angle

A

4 bond pair
2 lone pair
square planar
90

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22
Q

what is electronegativity

A

ability for an atom atom attract electrons towards itself in a covalent bond

23
Q

what is the most electronegative element

24
Q

how does a bond become polar

A

if atoms in a covalent bond have a difference in electronegativity

a bigger diff means more polar

25
Q

are hydrocarbons classed as polar

A

no
very small diff in electronegativity

26
Q

why is CO2 not polar

A

symmetrical polar bonds
no overall polarity

27
Q

list intermolecular forces in order of decreasing strength

A

h bonding
permenant dipole dipole
London

28
Q

what are London forces/ induced dipole dipole

A

any molecule/ atom with electrons can form a dipole when near another atom/ molecule

electrons in molecule/ atom can move from one end to another

dipole interaction destroyed when atoms/ molecules move away

29
Q

what are permanent dipole dipole forces

A

weak electrostatic forces between molecules with a polarity

30
Q

what is a test for polar molecules

A

charged rod near a stream of a polar liquid
liquid bends towards rod

31
Q

what is h bonding

A

when hydrogen forms a bond w the lone pair on N/O/F (3 most electronegative elements)

32
Q

simple molecular eg

33
Q

giant ionic eg

A

NaCl
CaO
MgBr2

34
Q

is ice or water more dense

35
Q

what are acids

A

proton donors

36
Q

what are bases

A

proton acceptors

37
Q

what is an alkali

A

soluble base

38
Q

weak acid eg

39
Q

strong acid eg

A

hydrochloric
nitric
sulfuric

40
Q

weak base eg

41
Q

strong base eg

A

sodium hydroxide
potassium hydroxide

42
Q

what are polyprotic acids

A

donate more than one proton

43
Q

acid + base =

A

salt + water

44
Q

NH3 + H2O =

A

NH4+ + OH-

45
Q

metal + acid =

A

salt + hydrogen

46
Q

metal oxide + acid =

A

salt + water

47
Q

metal hydroxide + acid =

A

salt + water

48
Q

metal carbonate + acid =

A

salt + water + carbon dioxide

49
Q

indicators eg

A

phenolphthalein
acid- colourless
alkali- pink

methyl orange
acid- red
alkali- yellow

50
Q

method for making a standard solution

A
  1. weigh solid precisely w a balance and weighing boat
  2. transfer to beaker, wash any solid left into beaker w deionised water
  3. fully dissolve solid w deionised water, stir
  4. transfer solution to volumetric flask using a funnel, rinse beaker and glass rod w deionised water
  5. deionised water to fill volumetric flask till graduation line, use pipette
  6. invert flask to thoroughly mix solution
51
Q

oxidation number of aluminium

52
Q

systemic name of ClO2-

A

chlorate (III)

53
Q

exceptions to Aufbau principle

A

Cr 3d5 4s1
Cu 3d10 4s1

54
Q

equation w 24dm3

A

24dm3 =
volume dm3 /
moles

chem (5 decks)

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