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Chemistry > TEST > Flashcards

TEST Flashcards

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1
Q

when a solid is heated

A

When a solid is heated, particles vibrate faster about a fixed point causing particles to move further apart and so solid expands

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2
Q

when particles get sufficient energy

A

When particles gain sufficient energy to overcome strong forces of attraction, they move out of their fixed position and can slide over each other in a continuous random motion – solid has melted.

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3
Q

particles in liquid

A

Particles in liquid have energy to move around but are still close to each other and do not have enough energy to overcome the forces that hold them close to each other.

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4
Q

if more heats supplied

A

If more heat’s supplied, particles move faster until they have enough energy to overcome the forces of attraction. Particles escape the liquids surface and move around in continuous rapid motion – the liquid has boiled

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5
Q

in the vapour

A

In the vapor, the particles move in rapid random motion. This movement is due to collision of vapor particles with air particles.

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6
Q

solid

A 
Strong forces of
attraction between
particles
 Fixed pattern
(lattice)
 Atoms vibrate but
can’t change
position ∴ fixed
volume and shape
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7
Q

liquid

A 
Weaker attractive
forces than solids
 No fixed pattern,
liquids take up the
shape of their
container
 Particles slide past
each other.
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8
Q

gas

A 
Almost no
intermolecular
forces
 Particles far apart,
and move quickly
 Collide with each
other and bounce
in all directions
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9
Q

endothermic heat energy gained

A

melting
boiling
sublimation

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10
Q

diffusion

A

Diffusion is the spreading of one substance through another from a
region of high concentration to a region of low concentration due to
the continuous random motion of particles.

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11
Q

it is endothermic because

A

energy is needed to overcome the force of attraction between molecules

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12
Q

gas at room temp

A

chlorine

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13
Q

non mettalic liquid at room temp

A

bromine

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14
Q

compound which is solid at room temp

A

sodium chloride

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15
Q

why is it towards hcl

A

because ammonia difusses faster and it has a lower mass

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16
Q

Type of chemical reacyion between ammonia and hcl

A

neutralization

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17
Q

copper oxide color

A

black

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18
Q

red brown solid

A

copper

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19
Q

drops of liquid

A

water

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20
Q

physical test to find thee liquid

A

its water so just check the boiling and freezing point 0 and 100 degree celcius

21
Q

arrangement of motion of atoms from condensation to solidification
gas liq sol

A

atoms of gas are randomly arranged and the atoms move very fast.slow down during condensation move slower.Atoms are close together and can slide over each other.During freezzing atoms further slow down and become more regularly arranged and can only vibrate

22
Q

when is it a liquid

A

when its mp is below room temp and bp is above room temp m.p is -79 degree celc and bp is 138 room temp is between boiling and melting point

23
Q

Factors that affect the rate of diffusion:

A

Temperature increases → rate of diffusion increases

o Lower density gas → rate of diffusion is higher

24
Q

Assesing purity from m.p./b.p:

A

Pure substances have a definite, sharp m.p./b.p.
o Substance+impurity has lower m.p. and higher b.p.
o More impurity means bigger change

25
Q

filtration

A 
Mixture goes in a
funnel with filter
paper, into a flask.
 Residue is insoluble
and stays at top.
 Filtrate goes through.
26
Q

Crystalization

A 
Some water in the
solution is evaporated
so solution becomes
more concentrated.
 A drop is placed on a
slide to check if
crystals are forming.
 Solution is left to cool
and crystallise.
 Crystals are filtered to
remove solvent.
27
Q

Simple distillation

A 
Impure liquid is heated
 It boils, and steam
rises into the
condenser
 Impurities are left
behind
 Condenser is cold so
steam condenses to
the pure liquid and it
drops into the beaker
28
Q

fractional distillation

A 
Removes a liquid from a mixture
of liquids, because liquids have
different b.p.s
 Mixture is heated to evaporate
substance with lowest b.p.
 some of the other liquid(s) will
evaporate too.
 A mixture of gases condense on
the beads in the fractional
column.
 So the beads are heated to the
boiling point of the lowest
substance, so that substance
being removed cannot condense
on the beads.
 The other substances continue
to condense and will drip back
into the flask.
 The beaker can be changed after
every fraction.
29
Q

The proton number increases

A

by 1 when you go to the right

30
Q

When you go one element down

A

you increase proton number

by 8 in the first 3 periods

31
Q

isotope

A

Isotopes: atoms of same element with different no. of neutrons
o E.g. Carbon 12 and Carbon 14.

32
Q

isotope medical

A

Medical use: cancer treatment (radiotherapy) – rays kill cancer
cells using cobalt-60

33
Q

industrial use

A

to check for leaks – radioisotopes (tracers)
added to oil/gas. At leaks radiation is detected using a Geiger
counter.

34
Q

element

A

that cannot be split into anything simpler, in a

chemical reaction. Each element has a unique proton number.

35
Q

mixture

A

two or more elements mixed together but not

chemically combined

36
Q

compouns

A

substance in which two or more different elements

are chemically combined

37
Q

metals non metals

A 
Metals Non-metals
Strong Brittle
Good conductors of heat &
electricity
Poor conductors of heat &
electricity (except graphite)
High m.p. and b.p. Lower m.p. and b.p. than metals
High density Low density
Forms basic oxides Forms acidic oxides
Forms cations in reactions Forms anions in reactions
Malleable and ductile
Sonorous
Some are magnetic
38
Q

alloy

A

Mixture of two or more metals or mixture of one or more

metal with a non-metal, to improve its properties

39
Q

ionic bonding

A

Strong electrostatic force of attraction between positive cations
and negative anions is called ionic bonding

40
Q

ionic property reason

A 
Property Reason
Form giant lattice Cations and anions attract
High m.p. and b.p. Strong bonds between ions
Don’t conduct electricity when
solid
Ions can’t move
Conduct electricity when
molten/aqueous
Ions can move
Usually soluble in water Not required
41
Q

covalent bonds

A

When atoms share 𝑒̅s to obtain a noble gas electron structure
 Covalent bonding takes place between non-metals only

42
Q

covalent compound property and reason

A

Property Reason
Low m.p. and b.p. Weak intermolecular forces of
attraction Usually liquid, gas or low m.p solid between molecules
Don’t conduct electricity No mobile ions/electrons
Usually insoluble in water Not required

43
Q

diamond

A 
Four bonds
 High m.p.
 Doesn’t conduct
 Used for cutting
as is srongest
known substance
44
Q

graphite

A 
Three bonds
 Made of flat sheets
 Held together by
weak forces so is
soft and
slipperyused as a
lubricant
 Conducts electricity
because it has one
free electron.
45
Q

silicon dioxide

A 
 Makes up sand
 Each Si is bonded to
4 oxygen atoms, and
each oxygen is
bonded to 2 silicon
atoms
 it has a high m.p.
and is hard, like
diamond
46
Q

Melting point: high

A

structure made up of strong covalent bonds

47
Q

strength

A

Strength: hard - exists in tetrahedral structure but graphite is soft

48
Q

mettalic bonding

A

metals are good conductors of electricity as free electrons can carry charge why good conductor of heat and electricity
strong electrostatic force of attraction between positive metal ions and free electrons is mettalic bond
Layers are held together by delocalized electrons.

Chemistry (7 decks)

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