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SA cycle sem 2 > CHEM > Flashcards

CHEM Flashcards

1
Q

Take in energy? (what reaction type)

A

Endothermic

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2
Q

Gives out energy (what reaction type)

A

exothermic

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3
Q

Increase in temp in surrounding/environment ((what reaction type)

A

exothermic

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4
Q

Decrease in temp in surrounding/environment (what reaction type)

A

endothermic

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5
Q

Heat is transferred from an object at high temp to a lower temp object until both of them are ……

A

equal

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6
Q

Bond breaking what type of reaction

A

Endothermic - absorbs energy

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7
Q

Bond forming what reaction type

A

exothermic - releases energy

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8
Q

Enthalpy

A

Change in Temp

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9
Q

Enthalpy and change in enthalpy symbol

A

H
ΔH

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10
Q

Bond Enthalpy

A

This is the energy required to break one mole of a specific bond type

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11
Q

If heat is absorbed (endothermic) ΔH is

A

positive

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12
Q

If heat is released (exothermic) ΔH is

A

negative

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13
Q

Entropy

A

Measurement of a system’s disorder or randomness

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14
Q

Entropy is most and least in

A

Most in gaseous
Least in solids

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15
Q

What all is required for a thing to burn

A

Heat, oxygen and fuel (substance containing carbon)

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16
Q

In which energy diagram is the product energy, less than the reactant energy

A

Exothermic (energy released is calculated by reactant energy - product energy

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17
Q

In which energy diagram is the product energy, more than the reactant energy

A

Endothermic (Energy absorbed is calculated by product energy - reactant energy)

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18
Q

Products of any combustion reaction

A

Water vapour and Carbon dioxide

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19
Q

Incomplete combustion

A

When there is insufficient oxygen in a combustion reaction and instead of carbon dioxide, carbon monoxide is formed

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20
Q

Ignition temp

A

Min temp required for something to catch fire

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21
Q

Bonding

A

The force of attraction between atoms so that they can be joined chemically

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22
Q

Why is bonding done

A

For an atom to become stable and make the outermost shell full

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23
Q

octet rule

A

the eight-electron arrangement in the outer electron shell of a noble-gas atom

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24
Q

Ions

A

Particles which carry a +ve or -ve charge

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25
Q

In bonding, what is used?

A

valence electrons

26
Q

Metals valency

A

metals only have 1,2 or 3 valence electrons which they lose, making them cations

27
Q

Types of bonding

A

Metallic, Ionic, Covalent

28
Q

Metallic bonding

A

Between two metals or alloys

29
Q

Alloys

A

A mixture of 2 or more metals

30
Q

Ionic or Electrovalent bonding

A

Between two ions which are always one metal and one non-metal

31
Q

Covalent Bonding

A

Between non-metals and non-metals where electrons are shared

32
Q

Properties of metals

A

Malleability
Durability
Good heat conductors
Good conductors of electricity
Sonorous
Shiny/Lustrous
Very high boiling and melting point

33
Q

Sonorous

A

When metals strike a hard surface, they produce a sound

34
Q

What is the sea of electrons in metals?

A

Outer electrons in metals separate from their atoms and become free and delocalised and form a sea of electrons. The atoms which lose these electrons become cations and the other free electrons allow for the movement of heat and electricity, making metals good conductors of both

35
Q

What happens when a metal is hit

A

Layers of strong and dense lattice slide over each other but do not break unlike ionic compound lattices

36
Q

Why is their sharing of electrons in covalent bonding

A

No atom wants to give their electrons, so they share to complete their octet

37
Q

Electronegativity

A

Ability of atoms to gain electrons

38
Q

Max amount of bonds carbon can form with itself

A

4

39
Q

Catenation

A

Catenation is the process of atoms of the same element linking together which is also called a chain

40
Q

Why are the oxides of carbon and silicon different even though they are in the same group?

A

The carbon atom is smaller than the silicon atom

41
Q

Which atom is found in millions of compounds

A

Carbon

42
Q

Lattice

A

a 3D arrangement of atoms, ions, or molecules in a crystalline solid.

43
Q

Name a gaseous fossil fuel

A

Natural Gas

44
Q

Name fuels obtained by distillation of petroleum

A

Gasoline, Kerosine, Diesel, propane

45
Q

Name two products obtained from petroleum which are not used as fuels

A

Bitumen and Lubricating Oil

46
Q

A mixture of liquid separate on an industrial scale other than petroleum

A

Ethanol and water

47
Q

If the oxidation number is positive, then electrons are

A

lost

48
Q

Which of these condust electricity during liquid state

Metallic compounds
Ionic compounds
Covalent compounds

A

Ionic compounds

49
Q

Which of these condust electricity during solid state

Metallic compounds
Ionic compounds
Covalent compounds

A

Metallic compounds

50
Q

Physical properties of Ionic compounds

A

High melting and boiling point
Solid at room temp
Poor conductors in the solid state, but good conductors in liquid state

51
Q

Physical properties of Covalent compounds

A

The state depends on compounds used
Boiling and melting points vary depending on the strength of covalent bonds and molecular weight
Poor conductors of electricity
Good conductors of heat - depending on the compound

52
Q

electrical neutrality

A

Electrical neutrality is when something has no net electrical charge.

53
Q

Allotropes

A

Matter, even if of the same element can exist in different physical states

54
Q

Allotropes of carbon and their structure

A

Graphite - Hexagonal structure with each atom connected with 4 others

Diamond - Tetrahedron shape with each atom connected with 4 others

55
Q

Silicia Alltrope shape

A

Each silicon atom is covalently bonded to four other oxygen atom in a tetrahedral arrangement.

56
Q

Why are metals good conductors of heat and electricity

A

loosely bound electrons roam freely throughout the metal. This is also known as the sea of electrons which carries heat energy and electricity across the metal and allows it to spread all over

57
Q

Which of the following is maleable and ductile:

Ionic bonds, Colvalent bonds or Metallic bonds

A

Metallic

58
Q

What makes a good fuel

A

Energy generated
Avaliability
How can it be stored
Cost
Toxicity
How easy is it to use

59
Q

Why do gases and liquids stay at the bottom of a fractional distillation tank?

A

Because they have a high boiling point and are much more dense

60
Q

Covalent network

A

a chemical compound where atoms are bonded by covalent bonds in a continuous network

61
Q

All allotropes are bonded with

A

covalent bonding

SA cycle sem 2 (3 decks)

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