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chemistry p1 Flashcards

(88 cards)

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1
Q

Compounds usually have what?

A

different compounds from their elements that make them

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2
Q

Atoms of different elements have one thing that is different and what is it?

A

Protons

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3
Q

Definition of an isotope

A

Atoms in same element that have a different number of neutrons

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4
Q

What is an ion

A

Charged particals that are formed when a molecule either gains or loses electrons

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5
Q

What is the mass number

A

number protons + number of neutrons

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6
Q

What is the atomic number

A

Number of protons

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7
Q

Mass number is what number on the element

A

The top number

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8
Q

What is the atomic number

A

The bottom number

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9
Q

How to find neutrons

A

mass number - number of protons

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10
Q

What is relative mass of all atoms of elemnt

A

average mass of the all atoms of an element

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11
Q

How to calculate relative atomic mass

A

percentage of isotope 1 x the mass of isotope 1 +mass of isotope 1 % of isotope 2 x mass of isotope 2
divide by
100

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12
Q

Simple distillation pratical

A

Soultion heated
liquid part evaporates and becomes a vapour
the vapour passes through condenser wher eits cooled
vapour condenses back to liquid
now seperated from solid

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13
Q

Fractional distillation

A

mixture is heated to lowest boiling pint
causes lowest boiling point liquid to evaporate
pass through condense - coll and condense
when all evaporated and condense- 2 diff liquids

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14
Q

Chromatography practical

A

Spot of mixture palced on pencil line near bottom of peice of paper of chromatgoraphy paper
Paper is placed upright in a solvent like wagter
solvent soaked up paper carrying diff componenets with it
diff componenets move at diff rates seperating them

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14
Q

practical of crystallation

A

gently heat mixuture in evaporation basin
some of solvent will evaporate making soultion concentrated
remove from the heat when crystals start to form
leave to cool and filter to remove excess liquid
leave crystals to dry

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15
Q

why is pencil used in chromatography

A

insouluble so doesent move

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16
Q

elements with similar porperties are put in what
and have same what>

A

groups
Downwards
electrons on outer shell

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16
Q

HIstory of model atom

A

Dalton model
solid sphere

Plum pudding model
JJ thompson

Rutherford experiment
Nuclear model

Bohr model
electorns orbit at specific distances

Discovery of proton 1920

Discovery of neutron 1932
James chadwick

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17
Q

Elements in same period have what?

A

same number of electrons shells
sideways

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18
Q

Mendeleev development of periodic table to solve atomic weight

A

arragned on similar porperites
horizontally with similar atomic weight
maintained patters by changing order of atomic weight

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19
Q

elements for positive ion

A

metal

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20
Q

element for negative ion

A

non metals

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21
Q

group 0 dont form what and what happens to boiling point

A

molecules
decreases as down the group

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22
Q

group 1

A

alkalie metals

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23
metal + water equals
metal hydroxide + hydrogen
24
what happens to reactivity for group 7 why
activity decreases harder to gain electron to fill outer shelll
25
melting and boiling point of group 7
increase down group because intermolecular forces stronger
26
halogens react with hydrgrognn
hydrogen halides form acidic when dissolved in water
27
transition metals group 1 properties
high melting point density and strength hard low melting point density and strength and soft
28
ionic covalent
metals and non etals non metals
28
whats ionic bonding
the strong electrostatic attraction between oppositely charged ions
29
ionic compounds are held by what
giant lattice structure of ions
30
ionic compounds properties
high metlign and boiling
31
strucutures of covalent
small molecules and giant covalent strucutres
32
polymers
large molecules repeated
33
small molecules equals
low melting and boiling
34
what is graphene
single layer of graphy and useful in electrical and strong
35
whats a fullerene and example
molecules fo carbon atoms with hallow shapes buckministeer
36
uses of buckminister
weak intermoleculer forces as a lubricant
37
use of nannopartical
medicine cosmetixs
38
equation for percentage by mass
total relative mass of atoms of that atom divide by relative fromula mass of compound times 100
39
mass equatio
relative formula mass times number of moles
40
relative formula mass equal
mass of 1 mole of a substance
41
concentratioon calculaton
mass divide by volume
42
what unit is conc.
dm3
43
percentage yield calcualtion
mass of product actually made divide maxium theoretical mass of product times 100
44
why do most reactions not have 100 percent yield
reaction may be reversible products lost during reaction
45
atomic enconomy equation and what is it
relative formula mass of desired product divide by sum of relative formula masses of all products time by 100
46
why high atom ecnomoy important
sustainable developemtn less waste - fewer natrual resources needed economic reasosn
47
metal + water observations
metal hydroxide + hydrogen metal dissolves and efferverscnece metal hydroxide formed as alkalie -purple
48
metal + acid observation
salt and hydrogen fizzing and metal disappears
49
the reactivity of metal means
how easily it form positive ions
50
metals less reactive than carbon...
be extracted from oxide by reducing with carbon
51
ions in soultion HCL H2SO4 HNO3
H+ and Cl- H+ SO4 2- H+ and NO3 -
52
how to neutralse an acid
alkalies (souluble metal hydroxides) bases (insouluble metal hydrzide and metal carbonates
53
Acid + metal carbonate equals
salt+ water + carbon dioxide
54
Acid + metal hydroxide
salt + water
55
neutralise acid of hydrochloric sulfuric and nitric
calcium carbonate sodium hydroxide magneisium hydroxide
56
what are salts made how to do it
acids reacted with solid insouluble substances the solid added to acid until no more reacts and excess solid is filtered to produce soultion of salt
57
pratical for crystallisation
choose acid and based for desired salt add dilute acid to flask heat gently using a bunsen burner add a small amount of base nad stir cotinue to add base until its inexcess filter to remove excess base pour remaning into evaporating basin use electrical heat or water bath to evaporate wate leaving crystals of salt
58
what ions do acids produce /alkalie in aqueos soultion
hydrogen ions hydroxide ions
59
how to carry out titration experiment
use a pipette to add 25 cm3 of alkalie to conical flask add few drops of methy orange fill biurette with acidd record starting volume of acid in burette add the acid drop by dop swirl between drops when a colour change is observed stop adding acid record final volume repeat until get concordant tires
60
what is titre and concordant tirtre
difference between final and inital volue of reading on biruette tires within 0.1 cm3 of eahc other
60
what is a strong acid?
a acid that is completely ionised in a aqueos soultion
61
what is a weak acid
a acid that is partially ionised in an aqueos soultion
62
what does a concentrated and dilute acid mean
a concentrated acid has alot of acid per unit volume a dilute has a small amount of acid per unit volume
63
at a given concentration
stronger acid equals a lower ph
64
as the hydrogen ion concentration increases by a factor of 10
the ph decreases by one unit
65
process of electroylsis
when an ionioc compound is melted or dissolved in water its ions are free to move through lqiuid or soultion these liquids and soultion conduct electricity and are called electryolytes when an electric current is passed through the electroylyte ions move to electrodes positive ions move to negative electroe - cathode negative ions move to positive electrode - the anode
66
what happesn to positive and negative ions
gain electrons ar=t cathode lsoe electrons at anode
67
when is electroylosis is used and
more reactive than carbon
68
alminuim extracted from alminium oxide by electroylosis
alminium oxide mixed with cryolite mixture heated utnil metls electroylosed using graphite electrodes alminium foms at cathode oxygen at anode
69
why is a mixture used for electroylote
reduces cost and lowrr melting temp
70
why must positive elctrode be continually replaced
oxygen is formed at anode which reacts with carbon anode to make co2 means anodes are oxides and need replacing
71
electroylosis of aqueos soultions h]why
is benefical over molten substances a sless energy needed working out product is harder because water breaks down and is present at cathhode hydrogen produced if metal more ractive at anode if halide ions present then halogen if no halide ions then o2 produced
72
examples of exothermic reactions
combustion neutralisation and oxideatin
73
exxamples of endothemric reactions
thermal decompoition
74
in exothermic
reactants higer than products
75
what is a cell
contain chemicals which react to rpoducce electricity
76
how to make a simple cell
connect 2 diff metals in contant with electroylte
77
a voltage produce by a cell depends on what
type of electrode electroylte
78
what is a battery
consists of two or more cell connecte din series for greater voltage
79
non rechargeable describe it and recharge
one reactant used up chemical reaction stop chemical reaction are reversible whe external current is apllied
80
how a fuel cell work and produced
fuel oxidies electrchemically within fuel cell to make a potential dfferent hydrogen oxidises to make water gains o2
81
hydrogen fuells celllls do what
provide alternative to battery and rechargeable cells and generate electricity with h20 and 02
82
half equation for negative an dpositive elctrode
2h2 and 4OH- equals 4H2) plus 4e- at anode 02 +2h20 +4 e- equals 4OH-
83
advanatges and disadvanatges of fuel cells
adv only waste produced is water dont need recharged hydrogen is difficult store highly flammable
84

scienice (7 decks)

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