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Science Class 10 NCERT > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Chemical reaction changes

A

State
Colour
Evolution of gas
Temperature

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2
Q

Decomposition of FeSO4

A

Fe2O3 + SO2 + SO3

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3
Q

NO2 Gas Colour

A

Brown

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4
Q

Pb(NO3)2 Decomposition

A

2PbO + 4NO2 + O2

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5
Q

AgCl Decompostion

A

Sunlight Ag + Cl2

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6
Q

AgBr

A

Ag + Br2

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7
Q

Colour of CuSO4

A

Blue

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8
Q

Colour of FeSO4

A

Greenish

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9
Q

Precipitate reaction

A

Na2SO4 + BaCl = BaSo4 + NaCl

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10
Q

BaSO4 properties

A

Insoluble and white

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11
Q

Cu on heating

A

Cu + O2 = CuO
CuO is black

(On heating)

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12
Q

CuO + H2

A

Cu + H2O
Black –> Brown surface

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13
Q

Sulphuric Acid

A

H2SO4

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14
Q

Nitric Acid

A

HNO3

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15
Q

Acetic Acid

A

CH3COOH

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16
Q

Acid + Metal

A

Salt + H2

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17
Q

Metal Carbonate/Metal Hydrogencarbonate + Acid

A

Salt + Carbon dioxide + Water

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18
Q

Base + Acid

A

Salt + H2O

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19
Q

Metal oxide + Acid

A

Salt + Water

Metal oxides are said to be basic oxides

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20
Q

Non-metal oxides + Base

A

Salt + Water

Non-metal oxides are said to acidic oxides

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21
Q

Body pH range

A

7 to 7.8

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22
Q

Acid rain pH

A

Lower than 5.6

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23
Q

-

Antacid

A

Milk of magnesia

Magnesium hydroxide

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24
Q

Tooth decay pH

A

Mouth pH less than 5.5

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25
Q

Vinegar contains

A

Acetic acid

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26
Q

Orange, Lemon contains

A

Citric acid

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27
Q

Sour milk (Curd)

A

Lactic acid

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28
Q

Ant and Nettle sting

A

Methanoic acid

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29
Q

Chlor-Alkali Process

A

Electricity is passed through brine soltution which makes Sodium Hydroxide

NaCl(aq) + H2O = NaOH + Cl2 + H2

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30
Q

Chlor-Alkali Process gas evolution

A

Chlorine gas is give off at the anode
Hydrogen gas at the cathode

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31
Q

Formation of bleaching power

A

Ca(OH)2 + Cl2 = CaOCl2 + H2O

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32
Q

Bleaching powder uses

A

Bleaching cotton
Oxidising agent
To make drinking water clean from germs

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33
Q

Formation of baking soda

A

NaCl + H2O + CO2 + NH3 = NH4Cl + NaHCO3

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34
Q

Decompositon of baking soda

A

Na2CO3 + H2O + CO2

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35
Q

Formation of Washing Soda

A

NaHCO3 –> Na2CO3 + H2O + CO2
Na2CO3 + 10 H2O –> Na2CO3.10H2O

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36
Q

CuSO4

A

CuSO4.5H2O is blue

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37
Q

Formation of POP

A

CaSO4.2H2O -heat 373K-> CaSO4.1/2H2O

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38
Q

Metal + Oxygen –>

A

Metal oxide

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39
Q

Metal + Water

A

Metal oxide + H2

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40
Q

Metal oxide + Water

A

Metal Hydroxide

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41
Q

Cold water reaction

A

Potassium, Sodiunm, Calcium(not too violently)

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42
Q

Why does calcium,magnesium float in water

A

H2 bubbles on surface

43
Q

hot water reaction

44
Q

steam reaction

A

Aluminium, iron, zinc

45
Q

Why doesn’t H2 not evolve when a metal reacts with nitric acid

A

HNO3 is a strong oxidizing agent. It oxidizes the H2 to H2O and itself gets reduced to nitrogen oxides

46
Q

Soft metals

A

Alkali Metals

(lithium, sodium, potassium)

47
Q

Amphoteric oxides

A

metal oxides which react with both acids as well as bases Al2O3 ZnO

48
Q

Atomic number of Helium

49
Q

Atomic number of Neon

50
Q

Atomic number of Argon

51
Q

Atomic number of Sodium

52
Q

Atomic number of Magnesium

53
Q

Atomic number of Aluminium

54
Q

Atomic number of Potassium

55
Q

Atomic number of Calcium

56
Q

Atomic number of Nitrogen

57
Q

Atomic number of Oxygen

58
Q

Atomic number of Fluorine

59
Q

Atomic number of Phosphorus

60
Q

Atomic number of Sulphur

61
Q

Atomic number of Chlorine

62
Q

Properties of ionic bonds

A

Solids and Hard because of strong force of attraction between ions
High melting and boiling points because of amount of energy required to break ionic attraction
Soluble
Molten ionic compounds conduct electricity

63
Q

Cinnabar

64
Q

Extraction of cinnabar

A

Roasting of HgS
HgS + O2 –> HgO + SO2
HgO –> Hg + O2

65
Q

Extraction of Copper

A

Roasting of Cu2S
Cu2S + O2 –> Cu2O + SO2
Cu2O + Cu2S –Heat–> Cu + SO2

66
Q

Extraction of Zinc

A

Roasting
ZnS + O2 –> ZnO + SO2
Calcination
ZnCO3 –> ZnO + CO2

ZnO + C(reducing agent) –> Zn + CO

67
Q

Extraction of Manganese

A

MnO2 + Al –> Mn + Al2O3 + Heat

68
Q

Extraction of Fe/ Thermit reaction

A

Fe2O3 + Al –> Fe + Al2O3 + Heat

Used to join railway tracks or cracked machine parts

69
Q

Extraction of Sodium/ Electrolytic refining

A

Impure metal is at the anode
Pure metal gets deposited at cathode
Anode mud gets deposited

Anode –> Positive terminal
Cl- –> Cl2 + 2e

Cathode –> Negative terminal
Na+ + e- –> Na

Metal salt is used at electrolyte

70
Q

Corrosion examples

A

Silver becomes black when exposed to sulphur in air(Silver sulphide)
Copper reacts with CO2 and gains a green coat(Copper carbonate)
Iron when exposed to moist air turns to rust(Fe2O3)

72
Q

Corrosion Prevention

A

Alloying
Galvinization
Painting
Greasing

73
Q

Amalgam meaning

A

If one of the metals in an alloy is mercury

74
Q

Brass composition

A

Alloy of copper and zinc

75
Q

Bronze composition

A

Alloy of copper and tin

76
Q

Solder composition

A

Alloy of Lead and tin

77
Q

Why can’t Carbon form ionic bonds

A

Gaining four electrons would be difficult for the 6 protons nucleus to hold 10 electrons
Loosing fouor electrons would require a large amount of energy

78
Q

Unqiue properties of carbon

A

Catenation
Capable of bonding with four other atoms

79
Q

Alcohol function group

A

— OH(ol)

80
Q

Aldehyde functional group

A

— C — H
||
O
(al)

81
Q

Ketone functional group

A

— C—
||
O
(one)

82
Q

Carboxylic acid

A

— C— OH
||
O
(oic)

83
Q

Combustion

A

Hydrocarbon + O2 –> CO2 + H2O + Heat and Light

H2O only present if H is present in hydrocarbon

84
Q

Oxidation reaction

A

Alcohols to carboxylic acids
CH3CH2OH — Alkaline KMnO4 + Heat — —> CH3COOH
Ethanol to Ethanoic acid

KMnO4 is a oxidising agent

85
Q

Addition Reaction

A

Unsaturated Hydrocarbon to saturated by adding H atoms
Nickel catalyst in presence of H2

86
Q

Substitution reaction

A

CH4 + Cl2 –> CH3Cl + HCl

87
Q

Ethanol reaction with sodium

A

Na + CH3CH2OH –> CH3CH3ONa + H2

88
Q

Heating ethanol at 443K/ reaction to give unsaturated hydrocarbon

A

CH3CH2OH –hot conc H2SO4–> CH2CH2 + H2O

conc sulphuric acid is dehydrating agent

89
Q

Esterification reaction

A

CH3COOH + CH3CH2OH —> CH3COOCH2CH3 + H2O

Easter plus water is formed

90
Q

Saponification reaction

A

CH3COOCH2CH3 —NaOH—> C2H5OH + CH3COONa

91
Q

Reaction of ethanoic acid by base

A

CH3COOH + NaOH –> CH3COONA + H20

92
Q

Reaction of ethanoic acid with carbonates and hydrocarbons

A

CH3COOH + Na2CO3/NaHCO3 –> CH3COONa + H2O + CO2

93
Q

Turmeric indicator colours

A

Acidic - Yellow
Basic - Red

94
Q

Red cabbage indicator colours

A

Acidic - Red
Basic -Green

95
Q

Hibiscus indicator colours

A

Acidic - Red
Basic - Green

96
Q

Methyl Orange indicator colours

A

Neutral - Orange
Acidic - Pink/Red
Base - Yellow

97
Q

Phenalphjthalein indicator colour

A

Neutral - Colourless
Acidic - Colourless
Basic - Pink

98
Q

Vanilla essence indicator

A

In basic medium no smell

99
Q

Carbon allotropes

A

Diamond
Graphite
Buckminsterfullerene

100
Q

Test between saturated and unsaturated hydrocarbons

A

Saturated hydrocarbons burns with clean blue flame
Unsaturated hydrocarbons produce yellow sooty flame

101
Q

Al plus water

A

Al2O3 + H2

102
Q

Iron plus water

A

Fe3O4 + H2

103
Q

Metal plus cold water

A

MetalOH plus H2 and energy

104
Q

Magnesium plus hot water

A

Mg(oh)2 plus H2

Science Class 10 NCERT (2 decks)

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