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chem Flashcards

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1
Q

who discovered protons

A

enerst. rutherford

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2
Q

who discovered neutrons

A

james chadwick

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3
Q

who discovered electrons

A

jj thompson

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4
Q

charge of an electron

A

1.60x10^-19C

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5
Q

CATIONS ARE

A

+VE

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6
Q

PLASMA

A

LIKE GAS BUT CONDUCTIVE

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7
Q

relative vapor density

A

mass of vol of gas/ mass of vol of hydrogen

mass of 1 mol of gas/mass of 1. mol of hydrogen

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7
Q

relative molecular mass

A

2 x relative vapor density

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8
Q

HETEROGENEOUS/HOMOGENOUS

A

Heterogeneous-trail mix
homogenous-salt water(evenly distributed)

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8
Q

boyles law

A

pv=k

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8
Q

charles law

A

k=v/t

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8
Q

gas lussacs

A

k=p/t

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9
Q

ideal gas law

A

PV=nRT

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9
Q

Electron affinity

A

energy changes when an electron is added to a neutral gas to form a negative ion-how much an atom likes to gain electrons

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10
Q

electronegativity

A

measure of an atoms ability to attract shared electrons

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11
Q

isobars

A

isobars are those elements that have a different atomic number but the same mass number.

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12
Q

deliquescence

A

garri
absorb water/moisture but form soluution
CaCl NaOH

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13
Q

Efflorescence

A

give out water of crystallisation when exposed to air

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14
Q

hygroscopic

A

eba
absorb moisture but do not form a solution
copper sulphate, sodium chloride, sulphuric acid

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15
Q

ionic bonding

A

metal+non-metal

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16
Q

covalent

A

non metal

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17
Q

metallic

A

metals

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18
Q

alkali metals

A

-stored under oil bc they react rapidly w/oxygen
-good conductors
-can be cut with a knife-soft
-low density,m.p,b.p
-m.p/b.p/density increase down the group

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19
Q

Halogens

A

-density/reactivity increase down the group
CL-yellow/green gas
Br-Red/brown liquid
I-grey/black solid

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20
Q

Summary of Dalton

A

-all matter is made of atoms which are indivisible
-atoms combine in simple ratio
-

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21
Q

JJ Thompson

A

-plum pudding model
-couldn’t explain how +ve charged ions hold the electrons
-cathode ray experiment

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22
Q

Rutherford

A

-gold foil experiment
-atom is made of mostly empty space
-couldn’t explain stability of atom/arrangement of ions

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23
Q

BOHR

A

-Father of quantum physics
-electrons revolve around the nucleus/in a stationary orbit
-electrons lose/gain by jumping to another orbit
-violates Heisenberg uncertainty principle

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24
Q

Orbitals

A

principal(N)-energy level,size of orbital
Azimuthal(L)-sub level,shape of. orbitals
magnetic(M)-no of orbitals
spin(s)-direction of spin

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25
Q

uses of radioactive elements

A

Uranium-use in nuclear power + weapons
Potassium-found in food-essential for life
Radium-luminous plants

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26
Q

Properties of Ionic bonding

A

-large electronegativity>1.5
-solid @ room temp
-doesnt dissolve in non polar solvents
-high m.p/b.p

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27
Q

Properties of covalent bonding

A

-small electronegativity<1.5
-gas/liquid @ room temp
-insoluble in polar(water/ethanol/ammonia) solvents
-low m.p/b.p

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28
Q

What is a polar molecules

A

molecules with unequal sharing of electrons
A polar molecule is a molecule in which one end of the molecule is slightly positive, while the other end is slightly negative.

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29
Q

hydrogen bond

A

-weak attractive forces btw molecules in which hydrogen is covalently linked to a highly electronegative element
-HCL,HF,c2h3OH

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30
Q

van der waals forces

A

weak forces btw polar molecules

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31
Q

use of artificial radioactivity

A

-used to bombard stable nucleus to emit radiation

32
Q

features of Alpha particles(8)

A

-Helium nucleus
-large mass+momentum
-low velocity+penetrating power
-most ionising
-produces florescence with Zinc sulfide
-stopped by a sheet of paper

-only harmful if inhaled/ingested-biological damage
-uses:smoke detectors+treatments for cancer

33
Q

features of beta particles

A

-fast moving electrons
-small mass+momentum
-high velocity+penetrating power
–produces florescence with Antracine
-stopped by aluminium foil

-can penetrate the skin, harmful if inhaled/ingested-skin burns/damaged tissues
-uses:medical diagnosis, radiotherapy , tracers

34
Q

features of gamma ray

A

-electromagnetic radiation
-neglible mass+momentum
-very high velocity+penetrating power
-low ionising
–produces florescence with NaI/ZnS
-stopped by LEAD

-damage to internal organs/DNA
-uses: medical imaging[PET scans], cancer treatments, sterilising medical equipment

35
Q

Radiation detectors

A

-geiger muller counter
-scintillation counter
-diffusion cloud chambers

36
Q

uses of radioactivity

A

-energy production
-archeology+geology
-food preservations
-environmental monitoring

37
Q

what reduces and stops rate of fission

A

graphite/heavy water-reduces rate of fission
Cadium/boron rods-stops neutrons

38
Q

nuclear fusion vs fission

A

Fission is the splitting of a heavy, unstable nucleus into two lighter nuclei, and fusion is the process where two light nuclei combine together releasing vast amounts of energy.

39
Q

what does alkaline pyrogallol remove

A

0xyegn

40
Q

what does sodium hydroide remove

A

C02

41
Q

what does CONC TETRAOXOSULLPHAATE (VI) remove

A

WATER

42
Q

Composition of air and its uses

A

78% -N-ammonia, growth of plants, fertilisers
21%-02-respiration+combustion
0.03%-C02-fire extinguishers, photosythesis
1%-Argon+ neon-electric lamps, welding/neon lights+aerodrome
krypton- photographs, filling gas+ fluorescent lights
hydrogen-haber process/filling balloons/ hardening oil/ hydrogen bomb

43
Q

water+metal=

A

metal oxide+H2

44
Q

WATER+NON METAL=

A

ACIDS+H2

45
Q

WATER+OXIDES

A

=ALKALOIDS

46
Q

TREATMENT OF WATER(7)

A

1.coagulation/flocculation- of alum to make tiny impurities clump
2.sedimention
3.filtration
4.disinfection - chlorine is added
5.Iodination-to prevent goitre
6.Flourination- prevent tooth decay
7.Liming-slaked lime to improve taste/remove hardness

47
Q

permanent hardness

A

-caused by MgS04/CaS04
REMOVED BY Na0H/washing soda

48
Q

Temp hardness

A

-caused by Ca(HC03)2/Mg(HC03)2
REMOVED BY BOILING/Adding slaked lime/Nh3

49
Q

formula for molarity+solubility

A

molarity=mols of solute/litres or kg of solvent

solubility= 1000n/v[cm3]

50
Q

factors. affecting. solubility

A

-Temp:solubility in solids increase, fluids decrease
-pressure solubility. increases in gases

51
Q

true solution vs. false solution

A

true solution: can’t scatter light, very small particles, homogeneous

false-not fully dissolved but cant be seen with eye, scatter light, heterogenous

52
Q

soluble salts

A

-chloride salts except lead,mecury+silver
-sulfates except barium, calcium,lead
-hydroxides[only sodium,K,Ba,Ca]

ALL SULFIDE/ PHOSPHATES/ CARBONATES ARE INSOLUBLE

53
Q

raw materials of
-plastic
-cement
-paper
-glass
-steel

A

-plastic: photochemicals from crude oil
-cement:limestonne
-paper:sodium sulphate
-glass:sand,limestone,sodium sulphate, sodium carbonate
-steel:iron ore, carbon

54
Q

raw materials of
-textile
-soap
-margarine
-fertiliser
-petroleum
-ceramics

A

-textile:cellulose from cotton, petrochemical
-soap: fats+oils, KOH, NaOH
-margarine:vegetable oils
-fertiliser:tetraoxophosphate potash,NH3
-petroleum: CRUDE OIL
-ceramics: Silica, oxides Mg,Al,Chronium

55
Q

fine chemicals

A

-required in small quantities
–purity is of high importance
-active pharmaceuticals ingredients, fragrance, specialised polymers

56
Q

Air pollutants + effects:

A

-hydrogen sulfide~respiratory issues
-C02~headaches, dizziness, possible death
-S02-respiratory issues
-nitrogen oxides~smog+. acid rain/ respiratory issues
-chlorofluorocarbons ~depletion of ozone layer
-dust~respiratory problems/ formation of smog

57
Q

Heavy chemicals

A

-required in large quantities

58
Q

solution for oil spillages

A

-pouring detergents
-using bacterial to digest the spilled oil
-burning

59
Q

what are the types of oxides

A

Acidic:non-metal+oxygen
Neutral: doesnt react w/ bases or acids
basic: metal + oxygen-copper oxide/calcium oxide

60
Q

methyl orange indicator

A

acid- red
base-yellow

61
Q

phenolphthalein

A

acid-colourless
base-pink

62
Q

oxidation

A

addition of. oxygen,increase in oxidation num, removal of hydrogen, loss of electrons,

63
Q

reduction

A

removal of. oxygen, decrease in oxidation num, addition of hydrogen, gain of electrons,

64
Q

What is the reaction of a reducing agent and KMnO4/K2Cr207

A

KMnO4-purple to colourless
K2Cr207-orange to green

65
Q

does reduction/oxidation occur at the anode/cathode

A

anode(+)-oxidation
cathode(-)-reduction

66
Q

uses of electrolysis

A

extraction of metals
purification of metals
electroplating

67
Q

faradays laws + formulas

A

1)mass of substance deposited is directly proportional to the quantity of electricity passed through electrolyte
2)Masses of diff substances deposited by the same quantity of electricity is directly proportional to the chemical equivalent weight

Mass=molar mass x current x time/charge x faradays constant
m=MIT/qf

m=zit

68
Q

Explain how purification of metals occur

A

anode:impure metal
cathode:tiny strip of pure metals
electrolyte most contain the metal ions

69
Q

Explain how electroplating of metals occur

A

anode:coating metal
cathode:metal to be coated
electrolyte- salt containing coating metal ions

70
Q

how to prevent rusting

A

-painting
-galvanisation
-electroplating

71
Q

what is the difference between primary electrochemical cells and secondary ones

A

primary-can’t be recharged-reaction that generates current that is irreversible
-e.g: daniel + Leclanche cells

secondary-can be recharged
e.g:lead cell accumulator+alkaline accumulator

72
Q

what are the anode/cathode/electrolyte/depolarizer/uses of primary electrochemical cells

A

Daniel-Zinc rod/copper rod/ zinc or copper sulphate/ -/ experiments

Leclanche-zinc rod/carbon rod/ ammonium chloride/Mn0/ Torch light + battery

73
Q

what are the anode/cathode/electrolyte/depolarizer/uses of secondary electrochemical cells

A

Lead Acid accumulator- lead metal/ lead oxide/h2s04/ car battery

74
Q

Entropy + gibbs free energy

A

-degree of randomness -s
-Gibbs free energy-energy available for doing work

75
Q

Endothermic + exothermic

A

Endothermic(+enthalpy change)-energy taken from surroundings. -electrolysis, thermal decomposition, First stage of photosynthesis

Exothermic(-enthalpy change)- gives out energy to environment-combustion, oxidation, neutralisation, condensation

76
Q

when is a reaction spontaneous

A

if the change in gibbs free energy=-ve, change in enthalpy =-ve change in entropy=+ve

77
Q

formula for rate of chemical reaction + active mass

A

R=conc of product/change in time
active mass= conc x activity coefficient

78
Q

what is equilibrium constant?

A

Ek=Forward equillibrium/backward equillibrium

79
Q

strong electrolytes

A

HCL
HN03
NAOH
KOH
NACL
H2SO4

80
Q

NON ELECTROLYTES

A

UREA
ETHANOL
SUGAR
benzene

81
Q

WEAK ELECTROLYTES

A

organic acids
amines
nh3
water

82
Q

how does an increase in temp affect exothermic/endothermic reactions

A

exo-shifts to reactants
endo-shift to products

83
Q

what is the test for protein

A

Xanthopreitic test for the presence of protein, when conc nitric acid is added to the drop, an intense yellow colouration is observed.

It contains all the functional group of protein which includes the amino, alkanol and the carboxylic group.

chem jamb (3 decks)

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