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Exam revision Flashcards

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1
Q

1 carbon
2 carbons
3 carbons
4 carbons
5 carbons

A

meth-
eth-
prop-
but-
pent-

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2
Q

6 carbons
7 carbons
8 carbons
9 carbons
10 carbons

A

hex-
hept-
oct-
non-
dec-

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3
Q

branch with one group
branch with two groups
branch with three groups

A

methyl
ethyl
propyl

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4
Q

What does M stand for and what is it?

A

It is the molar mass (gmol-1) it can be found out using Ar(x)+Ar(b)
(Ar is found on the periodic table)

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5
Q

What does n stand for and how can it be found?

A

Number of moles(mol)
It can be found using n=m(mass g)/M(gmol-1)
n=N/NA

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6
Q

What does N stand for and how is it found

A

Number of particles
If we know the mole(n)
N=nxNA

If we know the mass(m)
1.n=m/M
2.N=nxNA

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7
Q

What does m stand for and how can it be found

A

It is mass(g)
If we know the number of particles (N)
1.n=N/NA
2.m=nxNA
If we know the mole(n)

m=nxNA

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8
Q

what is NA

A

Advogadros constant (mol-1)
6.02x10^23

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9
Q

Empirical formula

A

Composition/ mass found in pt
Then divide by the smallest answer
times by something that can make them full numbers if needed

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10
Q

when asked for the amount of substance

A

mol
n=N/Na

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11
Q

when asked for the number of molecules

A

N=nxNa

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12
Q

when asked for the number of atoms

A

N=(how much elements there are ex. H2O=3)xnxNa

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13
Q

Ar formula

A

(no. of pt)x(abundance)/100

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14
Q

percentage composition

A

(how much of the element) /the no. found on pt x 100

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15
Q

Electronegativity trends

A

High for non metals
Group 18 no electronegativity
Less pull when valence electrons further from nucleus

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16
Q

First Ionisation Trends

A

Decreases going down a group
Increases across a period

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17
Q

Reactivity trends

A

Group 1 most reactive followed by group 2 in the metals but in the non metals it’s group 17 followed by group 16
Group 18 no reactivity
The reactivity of an element belonging to metals increases on moving from top to bottom in a group of the periodic table. While moving from top to bottom in a group of the periodic table, the reactivity of non-metals decreases.

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18
Q

Atomic radii trends

A

Decrease from left to right across a period to group 18
Increase as you go down a group

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19
Q

Electronegativity trends

A

Group 18 has no electronegativity
Increase across a period and up a group

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20
Q

intramolecular

A

bonds that hold atoms within molecules
-covalent bonds
-ionic bonds

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21
Q

intermolecular

A

bonds that occur between molecules and hold them together
-h-bonding
~FON
-dipole-dipole
-dispersion forces

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22
Q

metallic bonding properties

A

-due to mobile electrons being able to reflect light they are lustre
-electrons are able to gain kinetic energy in hotter areas of the metal and are able to transfer it to other parts of the metal lattice (bc of free moving electrons they bump into each other=transfer)
-high density because metallic lattices are closed packed
- high melting point and hardness:
–strong bonding
–increase the number of outer shell electrons (bc greater attraction force between the cation and the electrons)
-when an electrical field is applied one end becomes positive and the other negative .electrons experience a force toward the positive end (this is called an electric current )
-not brittle malleable

23
Q

Graphite Properties

A

is solid with a high melting point due to strong covalent bonds

conducts both electricity and heat due to the presence and movement of delocalised electrons

is slippery to the touch because weak dispersion forces between layers allow the layers to slide over each other

has a metallic sheen due to the interaction between light and the delocalised electrons.

24
Q

Mass number

A

Number of protons-number of neutrons

25
Q

Neutrons

A

Mass number-atomic number

26
Q

Metallic character

A

Easily lose electrons, conducts electricity and shiny

27
Q

Non- metallic character

A

Non- metals, gain electrons

28
Q

how many electrons can occupy subshells 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f

A

1s=2
2s=2
2p=6
3s=2
3p=6
3d=10
4s=2
4p=6
4d=10
4f=14

29
Q

Maximum number of electrons for each shell

A

Shell1:2
Shell2:8
Shell3:18
Shell4:32

30
Q

covalent bond=

A

non-metals

31
Q

where are the metals, metalloids and non-metals

A

metalloids =boron, silicon, arsenic, tellurium, astatine, germanium and antimony
on the right side of the metalloids are the non-metals
on the left side of metalloids are metals

32
Q

with electron subshell configuration when do you stop

A

stop on the element

33
Q

reactivity=

A

how easy it is for an atom to lose of gain electrons

34
Q

allotropes

A

two or more physical forms an element can exist example graphite diamond

35
Q

when an element is in its excited state…

A

it means it is not fully filled the shells and moved on to other shells

36
Q

why are metals more reactive than non metals

A

because are more reactive than non-metals because have many free electrons to give away .

37
Q

what info does 3 occupied electron shells and 2 valence electrons give us

A

that the element is in period 3 and group 2

38
Q

how to find out which element has a larger atomic radius

A

the one with more electron shells occupied

39
Q

what does unsaturated mean when referring to hydrocarbons

A

is one that has one or more carbon to carbon double or triple bonds

40
Q

what ion does non-metals form

A

negative ion

41
Q

when something is a lattice what does it experiences

A

intermolecular forces

42
Q

what are alkanes and alkenes (bond? polarity)

A

they are non polar and experience dispersion forces

43
Q

molecular formula

A

molar mass of a compound / molar mass of one empirical formula unit the answer is what u times the empirical formula by

44
Q

what is the ratio of calcium ions to fluorine ions

A

each calcium atom needs to lose 2 electrons to achieve stability but each fluorine needs to gain one so two fluorine to atoms to 1 calcium

45
Q

if it gains 2 it comes…
if it loses 2 it becomes

A

negative
positive

46
Q

atomic number represents

A

the electrons and protons neutrons are diff

47
Q

vitamin C contains 54.5% oxygen by mass. how many atoms of oxygen in one molecule of vitamin C? when given the gmol and percentage

A

Step 1: Calculate the mass of oxygen in one mole of Vitamin C
Since Vitamin C contains 54.5% (divide by 100) oxygen by mass, we can find the mass of oxygen in one mole of Vitamin C by multiplying the molar mass by the percentage of oxygen.
Mass of oxygen = 176.14 g/mol x 0.545 = 95.95 g/mol

Step 2: Calculate the number of moles of oxygen in one mole of Vitamin C
To find the number of moles of oxygen, we need to divide the mass of oxygen by the molar mass of oxygen.
Number of moles of oxygen = 95.95 g/mol / 16.00 g/mol = 6 moles

48
Q

how to find the molar mass of the empirical formula

A

empirical formula:
C5H6
(12x5)+(6x1)= molar mass

49
Q

ionic bonding properties

A

The properties of ionic bonding include high melting and boiling points, poor conductivity in the solid state, and high conductivity in molten/ liquid form

50
Q

tetrachloromethane

A

Tetrachloroethene has a higher boiling point than tetrachloromethane because it has stronger intermolecular forces.

51
Q

properties of hydrocarbons

A

-non-polar
-strong intramolecular bonds=covalent
-intermolecular forces are weak dispersion forces
-larger molecules high boiling points due to strong forces

52
Q

haloalkanes:
BR
I
F
C

A

bromo-
iodo-
flouro-
chloro-

53
Q

what do you add when naming a alcohol

A

-ol is the ending ex. ethanol

54
Q

carboxylic acids ending

A

-onic acid

Chemistry (13 decks)

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