C2

Front 1

Whatare the masses and charges of these parts of an atom?

· Proton

· Neutron

· Electron

Back 1

Protons= +ve (mass1) Neutrons= neutral (mass1) Electrons= -ve (mass1/2000th)

Front 2

Why do atoms usually haveno overall electrical charge?

Back 2

Atomsusually have no overall charge because they have equal numbers of protons (+ve)and electrons (-ve), which cancel one another out

Front 3

Allatoms of a particular element (e.g. carbon) all have the same number of what?

Back 3

Protons

Front 4

Whatare the following numbers called?

Back 4

a= relative atomic mass b= atomic number

Front 5

Whatdo the numbers tell you about the atom?

Back 5

a= relative atomic mass – the number of protons and neutrons in the atom

b= atomic number – the number of protons (usually the same as the number ofelectrons)

Front 6

Whatis an isotope?

Back 6

Anisotope is an atom with a different amount of neutronsY9

Front 7

Usethe periodic table to draw the electron structure of the following: -

· Neon

· Calcium

· Sodium

Howcan you tell which group these atoms are in?

Back 7

Thenumber of electrons in the outer shell is the same as their group number

Front 8

Theelectron structure of sodium can be represented as 2,8,1 – what does this mean? Represent these atoms: -

· Fluorine

· Oxygen

· Potassium

· Magnesium

Back 8

2,8,1means 2 electrons in the 1st shell, 8 electrons in the 2ndshell and 1 electron in the 3rd shell

Fluorine= 2,7

Oxygen= 2,6

Potassium= 2,8,8,1

Magnesium= 2,8,2

Front 9

How many electrons canoccupy the 1st and 2nd shell (energy level) of an atom?

Back 9

2in the 1st shell and 8 in the 2nd shell

Front 10

Whathappens to the electrons of 2 atoms when they chemically react?

Back 10

Duringa chemical reaction electrons are either given away, taken, or shared_

Front 11

Definethese terms: -

· Element

· Compound

· Mixture

Back 11

Element– a pure substance made from 1 type of atom only Compound– 2 or more elements chemically bound Mixture– 2 or more elements or compounds mixed together which are not chemically boundlass9^f

Front 12

Whatis an ion? Howare +ve ions formed? Howare -ve ions formed?

Back 12

Anion is an atom with a charge +veions have lost electrons -veions have gained electrons

Front 13

Explainhow the following atoms become ions (will they be +ve or –ve)?

· Potassium

· Magnesium

· Chlorine

· Oxygen

Back 13

Potassium– loses 1 electron (K+)

Magnesium– loses 2 electrons (Mg2+)

Chlorine– gains 1 electron (Cl-)

Oxygen– gains 2 electrons (O2-)

Front 14

Use diagrams to show howthese atoms for ionic bonds: -

Sodium + Chlorine

Back 14

Front 15

Describeand use a diagram to show the structure of ionic compounds

Back 15

Ioniccompounds have a giant structure – they are bonded to 6 other ions byelectrostatic bonds

Front 16

Whatare the melting and boiling points of ionic compounds like? Whyis this?

Back 16

Ioniccompounds have high melting points and boiling points – to melt them you haveto supply enough energy to break the 6 bonds attached to each ion

Front 17

Whathappens to the electrons when atoms form ionic bonds and covalent bonds? Whichis the strongest?

Back 17

Ionicbonds – 1 atom loses electrons and another gains electrons

Covalentbonds – electrons are shared

Anindividual covalent bond is stronger than an ionic bond

Front 18

Usediagrams to show how the following compounds are formed: -

· Hydrogen

· Oxygen

· Hydrogen Chloride

Back 18

Front 19

Usea diagram to show how water is formed

Back 19

Water(H2O)

Front 20

Howare the elements of the periodic table arranged?

Whatare the rows called?

Whatare the columns called?

Back 20

Elementsare arranged in order of atomic number

Rowsare called periods

Columnsare called groups

Front 21

What are the melting andboiling points of covalent compounds like? Explain why this is

Back 21

Covalentcompounds have low melting and boiling points (are often gases) are there is noattraction between the molecules

Front 22

Whydo elements in the same group have similar properties?

Back 22

Elementsin the same group have similar properties as they all have the same number ofelectrons in their outer shell'>CE1

Front 23

Which2 elements would be out of order in the periodic table if they were arranged byatomic mass instead of atomic number?

Back 23

Potassiumand ArgonA

Front 24

Whatare the symbols for these compounds?

· Calcium carbonate

· Sodium chloride

· Hydrochloric acid

Back 24

Calciumcarbonate – CaCO3

Sodiumchloride – NaCl

Hydrochloricacid - HCl

Front 25

Why do covalent compoundsnot conduct electricity when dissolved?

Back 25

Covalentcompounds do not conduct because they do no break down into ions

Front 26

Givethe names of 3 covalent compounds which have giant ionic structures? Whatis the structure of each like?

Back 26

Diamond– 4 carbon-carbon covalent bonds

Graphite– 3 carbon-carbon covalent bonds

Silicondioxide – 2 double silicon-oxygen covalent bonds

Front 27

Whydoes graphite conduct electricity?

Back 27

Graphiteconducts electricity because it is only bonded 3x (meaning there is adelocalised electron to pass the charge)

Front 28

Explainwhy ionic compounds have a giant structure

Back 28

Ioniccompounds have giant structures because the ions keep their charge and attractup to 6 other ions – forming a giant lattice

Front 29

Whatdoes monatomic mean and why are noble gases monatomic?

Back 29

Monatomic means an atom which only exists on its own (does not react) Noblegases are monatomic as they have a full shell and are un-reactive

Front 30

Whatdoes diatomic mean and why are elements such as the halogens, hydrogen andoxygen diatomic?

Back 30

Diatomic– atoms in pairs, e.g. H2 and O2

Halogenswill form diatomic molecules because they covalently bond with each other,forming pairs

Front 31

What is the bonding inmetals like?

Back 31

The bonding in metalscreates delocalised electrons (free to move and pass on electrical current)

Front 32

Whydo metals conduct electricity?

Back 32

The bonding in metalscreates delocalised electrons (free to move and pass on electrical current)