- solute heat solution until saturated crystals start to form, let solution cool separate with filter paper

Chem year 10 + 9 Flashcards by Aseena Saeed

chemical change

rearranged particles
irreversible

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limitations of the particle model

spheres
in elastic
solids
forces between
spaces between

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isotopes

same protons different neurtrons

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empirical formula

simplest form of ratio

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pure substances

sharp melting points
only one type of atom

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impure substances

melts over a range of
more then one type of atom
lower melting points
high boiling points

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Filtration

insoluble solids from a liquid
filter paper

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Crystallisation

solute
heat solution until saturated
crystals start to form, let solution cool
separate with filter paper

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distillation

solvent from solution
dependant on boiling points
condenser and boiling stuff

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fractional distillation

uses fractionating column
two or more substances in liquid state

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chromatography paper

stationary phase- paper
mobile phase- solvent

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chromatography TLC

stationary phase- thin layer of silica on glass plate
mobile phase- solvent

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gas chromatography

mobile phase- carrier gas (inert)
stationary phase- silica powder in metal column

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Rf value

distance travelled by substance
———————————————
distance travelled by solvent

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metals

shiny
ductile
malleable
good conductors
high melting and boiling points

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ionic compound

giant ionic lattice
strong electrostatic forces
metal and non-metals
high melting and boiling points

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simple molecules (covalent)

single bonds
gas state
low melting and boiling points
weak intermolecular forces

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giant covalent structures

covalent bond forces
large amount of energy

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diamond covalent bonds

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graphite covalent bonds

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silicon dioxide bonds

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polymers

made up of monomers

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structure of metals

positive ions attracted to delocalised electrons
electrostatic forces
high melting and boiling

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Mendeleev arrangement of periodic table

arranged elements in order of increasing atomic weight
grouped elements with similar properties

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current periodic table

order of increasing atomic number

allotropes

different forms of an element in the same state but with different atomic arrangements

nanoparticles

particle between 1nm and 100nm

conservation of mass

mass before and after a reaction will always be the same atoms can’t be created or destroyed

avagadros constant

6.02x 10(23)

moles formula

mass= molar mass x amount

limiting reactant

finding the moles and seeing which is less determines amount of product formed

exothermic and bonds

energy transferred to the surroundings bond forming

endothermic and bonds

energy transferred from surroundings to reaction bond breaking

oxidation

loss off electrons gain of oxygen

reduction

gain of electrons loss of oxygen

oxidising agent

gets reduced

reducing agent

gets oxidised

acids

red orange yellow ph 0- ph6

neutral

green ph-7

alkali

ph8-ph14 blues and purples

neutralisation

H+ + Oh- —> H2O

acid + base makes

salt and water

what is an alkali

base that’s dissolved in water

acids + carbonate

salt + water + carbon dioxide

acid + metal

salt + hydrogen

dilute vs concentrated acid

dilute acid contains less hydrogen ions concentrated acid contains more hydrogen ions

weak acids

partially ionises

string acids

full ionises

electrolysis

electric current passes through a compound causing a chemical change

solution in electrolysis is called

electrolyte

anode is

positive electrode

cathode is

negative electrode

intert meaning

unreactive

in electrolysis of a solution

if the positive charged substance is less reactive then hydrogen then it will be produced oxygen is produced unless there is an substance from group 7

electroplating

cathode—> object you want to coat anode—>. metal you want to coat the object with electrolyte is solution containing ions of the coating metal

Alkali metals

group 1 highly reactive softer as you go down density increases melting point decreases

halogens

group 7 diatomic weak intermolecular forces density + melting and boiling points increase reactivity decreases

noble gases

group 0 unreactive full outer shell nonmetals gas state at room temp forces get stronger/ boiling point increases density increases

transition metals

normal metal properties reactive stronger / harder have high density high melting points

less reactive then hydrogen

copper silver gold platinum

nanoparticle features

1-100 nm bigger then atoms high sa to v modify properties of materials effect on health isn’t fully understood

what bond holds polymer chains

strong covalent bonds

weak forces of polymers

held by weak intermolecular forces free to slide over each other yh er stretched easily low melting point

strong forces of polymers

covalent bonds high mp can’t be stretched cross links hold chain firmly together