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chemistry > principles of chem > Flashcards

principles of chem Flashcards

1
Q

solid

A
  • close
  • regular arrangements
  • vibrate in fixed position
  • strong force of attraction
  • fixed definite shape
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2
Q

liquid

A

– Close together
– a regular movement
– able to move/flow past each other
– fixed – take shape of container

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3
Q

gas

A 
– Spreadout
– far apart – irregular
– free to move randomly
– weak force attraction
– not fixed – expands to fill container
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4
Q

increase in temp.

A

– Gaining kinetic energy – move more
– energy is used to overcome force attraction between particles
– change in arrangement

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5
Q

evaporation vs. boiling

A
  • any temp.
  • slow
  • occurs at surface
  • certain temp.
  • fast
  • occurs throughout
  • bubbles
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6
Q

gas diffusion bromine gas

A
  • red brown vapour spreads throughout both gas jars (spread out so less concentrated)
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7
Q

liquid diffusion potassium magnate

A 
Purple crystal dissolves and diffuses 
Slower in liquids than gases
– particles have more energy
– move faster or more spread
– last trailer parks – less collisions
If you increase the temperature diffusion happen faster – particles have more KE
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8
Q

gas diffusion ammonia + hydrogen chloride gas

A

it’s a solid ammonium chloride form when gases meet
it’s not formed in the middle ( closer to HCl because NH three diffuse faster as it has smaller mass)
larger mass = slower diffusion

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9
Q

solute

A

solid that is dissolved in a solvent e.g. salt

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10
Q

solvent

A

Liquid the solute is dissolved in eg water

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11
Q

solution

A

mixture of solute + solvent eg salt water

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12
Q

saturated solution

A

when no more solute can dissolve in the solvent

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13
Q

insoluble

A

incapable of being dissolved in the solvent

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14
Q

solubility

A

A measure of how much solute can dissolve in a given volume of solvent at a given temperature measured in solute per 100 g of solvent

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15
Q

atom

A

smallest part of an element - cannot be broken down

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16
Q

molecule

A

two or more atoms chemically bonded together

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17
Q

giant lattice

A

A regular repeating arrangement of atoms or ions in a giant structure

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18
Q

element

A

pure substance made of only one kind of atom

- fixed melting / boiling point

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19
Q

compound

A

A pure substance that contains two or more types of atoms chemically bonded together
– fixed melting/boiling point

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20
Q

mixture

A

A substance that contains two or more types of elements/compounds not chemically bonded
– may melt/boil over a range of temperatures

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21
Q

metal + non metal >

A

__ _ide

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22
Q

metal + non metal + oxygen >

A

_ _ate

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23
Q

non metal + non metal >

A

_ _ide

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24
Q

ammonia

A

NH3

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25
Q

methane

A

CH4

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26
Q

distillation

A

soluble solid and solvent - keep both
– water boils leaving a soluble solid
– water vapour condenses because of cold water in condenser
– water is collected

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27
Q

fractional distillation

A

Mixture of miscible liquids with different boiling points – keep both
– heat to liquid1 boiling point
– mixture of liquid1 and some liquid2 water vapour rises + Condenses on beats hitting them up to boiling point1
- liquid1 no longer condenses only liquid2 does so liquid1 goes to condenser + drips into beaker

28
Q

filtration

A

separate insoluble solid + solvent - keep both

residue left in filter paper - filtrate goes through to beaker

29
Q

crystallisation

A

soluble solid and solvent – only keep solid
– heat until 2/3 as water is gone (saturated solution)
– test using glass rod (crystals form on rod)
- Cool and filter crystals

30
Q

chromatography

A 
mixture of different solutes
- draw pencil origin line + put dot of substance on 
- add solvent below base line
- remove before water reaches top 
- let it fry
result = chromatogram
31
Q

Rf

A

Distance solute travelled/distance solvent travelled (baseline –> solvent front)

32
Q

proton

A

mass 1
charge 1+
in nucleus

33
Q

neutron

A

mass 1
charge 0
in nucleus

34
Q

electron

A

mass 1/1800
charge 1-
in shells

35
Q

mass no

A

The sum of the number of neutrons and protons in an atomic nucleus

36
Q

atomic number

A

The number of protons in the nucleus of an atom (equal to the number of electrons)
Identity of an atom

37
Q

isotopes

A

atoms of the same element that have the same no. protons but a diff. no. neutrons

38
Q

relative atomic mass Ar

A

weighted average mass of one atom of an element relative to 1/12th of the mass of a C-12 atom

39
Q

how to work out Ar

A

(mass no. isotope1 x abundance1) + (mass no. isotope2 x abundance2)/ abundanec1 + abundance2

40
Q

ions

A

charged atoms – form when atoms lose or gain electrons to get a full outer shell

41
Q

cations

A

positive ions

42
Q

anions

A

negative ions

43
Q

silver ions

A

Ag +

44
Q

lead ion

A

Pb 2+

45
Q

zinc ion

A

Zn 2+

46
Q

hydroxide ion

A

OH-

47
Q

nitrate ion

A

NO3 -

48
Q

sulphate ion

A

SO4 2-

49
Q

carbonate ion

A

CO3 2-

50
Q

ammonium ion

A

NH4 +

51
Q

ionic bond

A

The electrostatic attraction between positive and negative ions

52
Q

ionic bonding

A

Metal and nonmetal
Gain/loss of electrons
Giant ionic lattice
Formula = ratio of anions to cations in the lattice

53
Q

physical properties of ionic compounds

A
  • High melting/boiling point – strong electrostatic attraction between anions and cations which requires lots of energy to break
    – poor conductor (solid) –ions can’t move
  • good conductor when molten or aqueous – has charged ions that can move
54
Q

why some ionic compounds have diff. melting points

A

The higher the charge of ions and the smaller the ions the stronger the electrostatic attraction between the ions

55
Q

covalent bond

A

electrostatic attraction
between the positive nuclei and shared pair of electrons
H- H

56
Q

covalent bonding

A

non metal + non metal
sharing of electrons
simple molecular or giant covalent structur

57
Q

simple molecular structure

A

atoms bonded covalently with weak intermolecular forces between molecules

58
Q

physical properties of simple molecular compounds

A
  • Low melting point – weak intermolecular forces are easy to overcome
  • Doesn’t conduct electricity – no charged ions/delocalised electrons – molecules are neutral
    – formula tells you how many atoms in each molecule
59
Q

why simple molecular covalent compounds change in melting point

A

melting points increase as the relative molecular mass of the molecules increase
– bigger RMM = stronger intermolecular forces between molecules
– more energy needed to overcome them

60
Q

fullerenes

A

Allotropes of carbon
– have spherical or cylindrical hollow shapes with rings of carbon atoms
– have simple molecular structure
E.g. buckminsterfullerene C60
Have low melting points/boiling point – weak intermolecular forces are easy to overcome

61
Q

giant covalent compounds

A

giant lattice structure
consisting of millions of atoms with strong covalent bonds between them
eg diamond graphite silicon dioxide

62
Q

diamond properties (like most others)

A

– Hard – strong covalent bonds between atoms
– very high mtp. – lots of energy needed to break strong covalent bonds
– don’t conduct electricity – no ions/delocalised electrons – neutral charged
– uses – drill heads/jewellery

63
Q

graphite properties

A
  • soft - Exists in layers that can slide over each other – weak forces between layers
    – very high mtp. – lots of energy needed to break strong covalent bonds
    – good conductors of electricity – contain delocalised electrons that can move throughout structure
    – uses – pencils/lubricant
64
Q

metallic bond

A

the strong attraction between positive ions and negative delocalised electrons

65
Q

metallic bonding

A

metal only

giant metallic lattice

66
Q

physical properties of metallic compounds

A
  • hi mtp. /bp. – lots of energy needed to overcome strong electrostatic attraction between cations and delocalised electrons
    – malleable and ductile – layers of irons can slide over each other
    – good conductors of electricity/heat –have delocalised electrons that are free to move throughout the structure
    
67
Q

why metallic compounds change in melting point

A

the higher the ions charge the more delocalised electrons and the stronger the electrostatic force which takes more energy to overcome

chemistry (17 decks)

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