Chemistry C4
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- Created by: aminah10
- Created on: 20-02-17 09:38
What does the nucleus contain
protons and neutrons
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What is the charge of the nucleus
positive because of the protons
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What charge is an electron
negative (-1)
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What is the mass of an electron
0.0005
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What is the charge of a neutron
0
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What does the mass (top) number tell you
no. of protons and neutrons
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What does the atomic (bottom) number tell you
no. of protons
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What is an isotope
Different forms of same element with same no of protons,but a different number of neutrons
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What do different isotopes of the same element have
same atomic number, different mass numbers
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how many electrons are allowed in each shell (123)
2,8,8
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If an element is in group 1 what does it mean
1 outer shell electron
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What do the periods(horizontal rows) tell you
How many shells they fill
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What is ionic bonding
When an atom loses or gains an electron to form a charged ion
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What will atoms with just 1 or 2 electrons in their outer shell do?
As they want full outer shells, the electron leaves as a POSITIVE ION, and will leap at the first passing ion with an opposite charge
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What will atoms with nearly full outer shells do (group 6 and 7)
Gain electrons to get a full outer shell, They become NEGATIVE ions
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Describe a giant ionic lattice
ionic bonds between metals and non metals, ions are not free to move, so DO NOT conduct electricity when solid. There are strong chemical bonds between all ions
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Properties of giant ionic lattices
High melting and boiling pt, v strong attraction between oppositley charged ions, need a lot of energy to overcome forces, when melted, ions free to move and will conduct electricity.
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What happens as you go DOWN group 1 metals
become more reactive
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Why do they become more reactive as you go down group 1
outer electron is futher from the nucleus ,outer electron is lost more easily, becuase less energy is needed to remove it
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Properties of alkali metals
Low melting point+Boiling pt Low density Very soft(can be cut w/ a knife)
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What charged ion do group 1 metals form when the electron is lost ( oxidised)
Form a 1+ ion (with a stable structure)
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What colour flame will lithium produce
red
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What colour flame will sodium produce
yellow/orange
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What colour flame will potassium produce
lilac
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What must you do with the wire before burning with an alkali metal and what colour flame is used
dip wire loop on hydrochloric acid to clean it and a BLUE flame is used
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What are halogens
Group 7 elements
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What happens as you go DOWN group 7 (reactivity)
halogens become LESS reactive- less inclination to gain extra electron when its futher away from the nucleus
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What do all halides do
react by gaining one electron to form a NEGATIVE ion
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What happens when you go down group 7
melting and boiling points increase
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What is formed when halogens react with alkali metals
metal halides (salts)
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When will halogens displace other halogens
When theyre more reactive ( futher UP the group)
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What structure do metals have
crystal structure
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What are metals held together by
metallic bonds
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What do metallic bonds allow?
outer electrons to move freely, therefore delocalised electrons throuought the metal
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Properties of metals
Hard,Dense,Lusterous, STRONG attraction between delocalised electrons and closley packed positive ions=strong metallic bond HIGH BP+HIGH MP- need a lot of energy to break strong metallic bond STRONG, but MALLEABLE(can change shape)
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How do metals conduct electricity
due to the delocalised electrons which carry electrical current, they also carry heat energy through metal
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When does the electrical resistance of some metals dissapear
When you make the temps cold enough - they become superconductors
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Why are superconductos useful
Without any resistance no electrical energy is turned into heat so none is wasted
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What temperature do metals start superconducting at? and why is it a problem
less than -256 degreesC!! Its very HARD and very EXPENSIVE
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What superconductors are scientists trying to develop now
Room temperature ones - ideally 20degrees C. So far theyve managed to get a metal oxide to conduct at -135 which is much cheaper
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What colour are Iron(II) compounds
LIGHT GREEN due to the transition metal ion it contains
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What colour is Iron(III) compounds
orange/brown due to the transition metal ion it contains
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What colour are copper compounds
blue due to the transition metal ion it contains
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What is thermal decomposition
Braking down a substance with heat
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What do all transition metal carbonates contain and do
CO3 and break down into a metal oxide( eg copper oxide) and carbon dioxide
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How can you prove thermal decomp has occured
colour change and test for CO2 by turning limewater milky
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What is a precipitation
Two solutions react and an insoluble solid forms
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What forms when a soluble transition metal compound reacts with sodium hydroxide
Forms an insoluble hydroxide ( precipitate) and sodium sulfate
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Name some transition metal carbonates
copper(II) carbonate =CuCO3, iron(II) carbonate=FeCO3, zinc carbonmate=ZnCO3, manganese carbonate=MnCO3
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What colour precipiate is Copper(II) hydroxide
blue
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What colour precipitate is Iron(II) hydroxide
grey/green
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What colour precipitate is Iron(III) hydroxide
orange/brown
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Where does the UK get its water from
SURFACE WATER: lakes,rivers,resivoirs GROUNDWATER:aquifers(rocks that trap water underground)
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Whys it important to conserve water
As all water resources are LIMITED depending on annual rainfall, and demand for water increases each year.
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Basic steps of surface water purification
mesh-sand filteration-sedimentation-chlorination (MSSC)
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Why does groundwater not need as much purification as surfacewater
groundwater from aquifers is usually quite pure
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Describe step 1+2 of water purification
Filteration- wire mesh stops twigs etc, sand beds filter out any other solid bits
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Describe step 3 of purification
Sedimentation- iron sulfate/aluminium sulfate is added to the water, makes particles clump together and settle to the bottom
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Describe step 4 of water purification
Chlorination- chlorine gas bubbled through to kill harmful bacteria/ microbes
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What can cause water hardness/ pesticides
If some impurities are DISSOLVED in the water and cannot be filtered out
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How do we know the water we drink is safe
Has to meet Strict Safety Standards
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What low levels of pollutatnts are still found in our water
Nitrates residue, Lead compounds, Pesticide residue
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How is nitrates residue dangerous
From excessd fertiliser run off -Prevent blood from carrying oxygen properly
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How is Lead compounds dangerous
from old lead pipes - poisonous
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How pesticides residue impurities get into our water
From spraying too near rivers and lakes
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How do dry countries get fresh water and what are cons of it
Distill sea water- needs loads of energy therefore is really expensive and not practical for producing large quantities
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What do you use to test for Sulfate ions
Barium chloride
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Describe steps to test for sulfate ions
add dilute hydrochloric acid , then add 10 drops of barium chloride- white precipitate=sulfate ions
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What is BaSO4
Barium sulfate - white precipitate
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What is used to test for halide ions
Silver Nitrate
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steps for testing for halide ions
dilute nitric acid , add 10 drops of silver nitrate, if halide ions are present, a precipitate will form
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what colour precipiate do chloride ions form
White
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What colour precipitate do Bromide ions form
Cream
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What colour precipitate do iodide ions form
Pale Yellow
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silver nitrate + sodium chloride --->
silver chloride + sodium nitrate
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silver nitrate+sodium bromide--->
silver bromide+sodium nitrate
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silver nitrate+sodium iodide--->
silver iodide+sodium nitrate
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sodium chloride=
NaCl
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Silver Nitrate =
AgNO3
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Sodium iodide=
NaI
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soduim nitrate=
NaNO3
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anything nitrate has
NO3
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Other cards in this set
Card 2
Front
What is the charge of the nucleus
Back
positive because of the protons
Card 3
Front
What charge is an electron
Back
Card 4
Front
What is the mass of an electron
Back
Card 5
Front
What is the charge of a neutron
Back
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