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A - Chemistry GCSE > Topic 1 - Key concepts > Flashcards

Topic 1 - Key concepts Flashcards

Key Concepts, States of matter and mixtures, chemical changes, extracting metals and equilibria

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1
Q

What were daltons ideas about how atoms have changed?

A

Dalton described atoms as solid spheres made up of different elements
JJ Thomson said they werent solid spheres but were positively charged “pudding” with electrons inside the dough (plum pudding)
Rutherford conducted gold foil experiment showed PPmodel was wrong as some of the alpha particle beam bounced back showing there was a positively charged nucleus but some passed through showing empty space
Bohr model is close to current model but shows electrons in circular shells with a nucleus in the middle

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2
Q

What are the relative charges and masses of subatomic particles?

A

-proton +1
mass of 1

-neutron 0
mass of 1

-electron -1
mass of 0.0005

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3
Q

Why do atoms have no overall charge?

A

because the number of protons and electrons are equal so the pos and neg cancel out
ions however have either lost or gained electrons so they do have a charge

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4
Q

how does the size of an atom compare to its nucleus

A

the whole mass of an atom is in the nucleus but compared to the whole atom the nucleus is tiny!

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5
Q

What is the atomic number

A

The number of protons ( and therefore electrons)

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6
Q

What is the mass number

A

the number of protons and neutrons

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7
Q

What is an isotope?

A

Same form of the same element but have a different number of neutrons. so they have different mass numbers! eg carbon 14.

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8
Q

How do you find the Ar of an element with many isotopes such as chlorine?

A

You would take an average of the mass numbers of each so 35.5

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9
Q

How do you find the Ar from isotopic abundances

A

multiply each realtive isotopic mass by its abundance and add up results
divide by sum of abundances. (Average)

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10
Q

How did mendeleev arrange the periodic table?

A

Put them into groups based off their chemical properties and put them into columns
then periods across
when putting in order of atomic mass a pattern appeared. however a few didnt fit and not all had been discovered so he left gaps.

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11
Q

What is the modern periodic table like compared

A

We now have more knowledge of isotopes and know many more elements which still fit in order of atomic number. rows are called periods and each new one represents a new shell of electons.

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12
Q

Where are the metals found?

A

in the middle and left

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13
Q

What does electronic configuration mean?

A

how each atoms electrons are laid out

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14
Q

what is an ion

A

when an atom loses or gains an electron

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15
Q

describe the general rule of how you would show if an atom had lost 2 electrons (with iron)

A

Fe2+

this means it has two more protons than electrons giving it a positive charge.

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16
Q

F- has a single negative charge it means….

A

theres one more electron than protons

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17
Q

Which groups are most likely to form ions

A 
1 &; 2 and 6 &; 7
group 1 make 1+
group 2 make 2+
group 6 make 2-
group 7 make 1-
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18
Q

What is the difference between an atom and an ion

A

An ion is a charged particle

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19
Q

How are cations and anions formed

A

cations (positive) form when atoms lose electrons so they have more protons than electrons

anions (negative) form when an atom gains electrons so there are more electrons than protons

20
Q

How do you work out the formula of an ionic compound

Using sodium chloride

A

sodium chloride
Na gives up its outer shell electron to chlorine to form Na+
chlorine gains an electron making it Cl-

21
Q

What is the structure of an ionic compound

A

Giant ionic lattices, regular lattice with strong electrostatic forces of attraction

22
Q

Name some properties of ionic compounds

A

High melting and boiling points due to strong electrostatic forces of attraction
dont conduct because ions cant move in fixed positions
dissolve easily in water as ions separate an move freely in solution.

23
Q

How do covalent bonds form

A

When a pair of electrons is shared between two atoms

24
Q

Give examples of covalent molecules

A

Water, methane, Hydrogen, CO2

25
Q

Name some properties of covalent molecules

A

very strong covalent bonds
forces of attraction are very weak
low melting and boiling points because of this so most are liquids/ gas at room temp
dont conduct as no free ions or electrons
no rule of solubility

26
Q

What is the structure of a polymer

A

Made up of covalently bonded carbon chains, made up of monomers than join together. eg polyethene

27
Q

Give examples of allotropes of carbon

A

diamond, graphine, graphite, fullerines

28
Q

What are some basic similarities / differences of simple covalent and giant covalent structures?

A

Giant have very high boiling and melting points as lots of energy is needed to break the strong covalent bonds
dont conduct as no charged particles apart from graphene and graphite
both are insoluble

29
Q

Describe fullerines and their uses

A

hollow tubes of carbon in pentagons or hexagons
can cage other molecules which is why theyre used to transport drugs.
large surface area so good catalysts in industrial
nanotubes have high tensile strength so used in sports equipment

30
Q

How are the particles arranged in metals as well as properties

A

-giant structure, regular structure
-outershell electrons are delocalised so carry current
-metallic bonding have strong electrostatic forces of attraction between them so high melting and boiling points (apart from mercury)
-dense
malleable

31
Q

What makes metals malleable?

A

Layers can slide over each other so they can be hammered or rolled.

32
Q

What are some typical properties of non metals

A

brittle, dull looking not shiny, non metals tend to gain electrons to form full outer shells, dont conduct

33
Q

Evaluate the models we can use to display structure and bonding

A

2D= + show atoms something contains and how joined
- dont show shape or sizes

Dot and Cross= + show where electrons and ions came from
-dont show you the size of the atoms or how arranged

3D= +show arrangement
-only show outer layer

Ball and stick= +good to visualise bonding and structures and are more realistic
-not correct scales, or show insides

34
Q

Chemical formula of water

A

H2O

35
Q

Carbon dioxide formula

A

CO2

36
Q

chlorine chem formula

A

Cl2

37
Q

ammonia chemical formula

A

NH3

38
Q

Hydrogen formula

A

H2

39
Q

Oxygen formula

A

O2

40
Q

(ions) Ammonium chemical formula

A

NH4+

41
Q

(ions) Nitrate

A

NO3-

42
Q

Sulfate ions

A

SO4 2-

43
Q

Hydroxide ions

A

OH-

44
Q

Carbonate ions

A

CO3 2-

45
Q

Whats the difference between empirical formula and molecular formula

A

empirical formula is the simplest ratio of atoms whereas molecular formula is is all the atomic masses added together

46
Q

What is the law of conservation in an enclosed system

A

Mass is always conserved so mass before equals mass after

47
Q

What is the law of conservation in a non- enclosed system

A

mass before doesnt equal mass after because some gas produced in the reaction could have escaped or oxygen from the air has reacted with the metal for example

A - Chemistry GCSE (11 decks)

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