Atomic structure and the periodic table

Question 1

Atoms

Answer 1

all substances are made up of tiny particles of tiny matter are called atoms which are building blocks of matter.

Question 2

Each atom is made up of

Answer 2

subatomic particles called protons, neutrons and electrons.

Question 3

The subatomic particles are located

Answer 3

in the nucleus of an atoms

Question 4

Isotopes are

Answer 4

atoms of the same element that have different numbers of neutrons

Question 5

Relative atomic mass equation is

Answer 5

Sum of 9=(isotope abundance x isotope mass number)/sum of abundance of all isotopes

Question 6

A compound is

Answer 6

a pure substance made up of two or more elements chemically combined and cannot be seperated physically.

Question 7

Elements are pure substances whilst

Answer 7

compounds are impure. Pure is only one element or compound which are not mixed with anything else.

Question 8

Ionic compounds contain

Answer 8

a metal and non-metal joined together as particles called ions.

Question 9

covalent compounds contain

Answer 9

only non-metals

Question 10

Ionic bonding is when

Answer 10

the metal atom loses electrons to form a positive ion and the non-metal atoms gains to form negative ions.

Question 11

Covalent bonding is when

Answer 11

each atom shares and electron with another atom.

Question 12

Covalent compound examples are

Answer 12

H2SO4 - sulfaric acid
NH3 - methane
MH3 - ammonia
HNO3 - nitirc acid

Question 13

Opposite charges of ions mean

Answer 13

they are strongly attracted to each other this is called ionic bonding.

Question 14

mixtures consists

Answer 14

of two or more substances that are not joined together.

Question 15

filtration seperates

Answer 15

insoluble solid from a mixture of solid and liquid .

Question 16

Filtration process

Answer 16

• filter placed in a filter funnel above a beaker . The mixture of insoluble solid and liquid is poured . Filter will only allow liquid particles to pass.

Question 17

crystallisation seperates

Answer 17

a dissolved solid from a solution

Question 18

crystallisation process

Answer 18

• pour the solution into an evaporating dish and gently heat the solution . Some of the solvent will evaporate and the solution will get more concentrated. When crystals are formed remove the dish from the heat and leave the solution to cool. The salt should start to form crystals as it becomes insoluble in the cold, highly concentrated solution. Filter the crystals out of the solution and leave them in a warm place in dry.

Question 19

simple distillation is

Answer 19

used to seperate a liquid and soluble liquid from a solution (e.g water from a solution of saltwater) or a place liquid from mixtures of liquids

Question 20

simple distillation process

Answer 20

the solution is heated and pure water evaporates producing vapour which rises through the neck of the round-bottom flask. The vapour passes through the condenser , where it cools and condenses turning into pure water which is collected in the beaker. after water is evaporated only solid solute will be left behind

Question 21

simple distillation can be used to

Answer 21

seperate the products of fermentation such as alchohol and water.

Question 22

Fractional distillation is used

Answer 22

to seperate a mixture of liquids .

Question 23

Fractional distillation process

Answer 23

• you can put mixture in a flask and stick a fractionating column on top. then heat it. The different liquids will have different boiling points. so they will evaporate at different temperatures. Liquid with lowest boiling point evaporates first. When temp on thermo matches boiling point of the liquid it will reach the top of the collum . liquids with higher boiling points may start to evaporate. when first liquid collected you raise the temperature for the next and the next.

Question 24

paper chromotography is used

Answer 24

to seperate substances that have different solubilities in a given solvent ..

Question 25

paper chromotography process

Answer 25

• pencil line + spots of sampled placed . paper lowered into solvent . Solvent travels up the paper by capillary action taking some of the coloured substance with it.

Question 26

Different substances in paper chromotography

Answer 26

have different solubilities so they will travel at different rates.

Question 27

JJ Thomas theory was

Answer 27

the ‘plum pudding model’ which was an atom depicted negative electrons embedded in a ball of positive charge.

Question 28

At the start John dalton described atoms as

Answer 28

solid spheres and discovered electrons.

Question 29

Ernest Rutherford consist

Answer 29

of empty space with nucleus having electrons orbitting around

Question 30

Ernest Rutherford experience was

Answer 30

he shot a beam of positively charged particles at a thin of sheet of gold foil and based on the plum pudding model. he expected they would pass through the foil or slightly deflected. Initially the deflected more than expected and small number went backwards.

Question 31

Rutherford came up with

Answer 31

the idea of the nuclear model of the atom .

Question 32

Bohr proposed that

Answer 32

electrons orbit the nucleus in fixed shells and aren’t anywhere in between.

Question 33

James chadwick carried

Answer 33

out an experiment which provided evidence for neutral particles known as neutrons.s

Question 34

In the early 1800s elements

Answer 34

were arranged by atomic weight

Question 35

Early periodic tables were

Answer 35

not complete and some elements were placed in the world group because elements were placed in order of atomic weight and did not take any account their properties

Question 36

Dmitrie Mendeleev

Answer 36

left gaps and predicted new elements. He mainly ordered them in atomic weight but did switch order for the properties aswell.

Question 37

The discovery of isotopes

Answer 37

confirmed that mendeleev was correct to not place elements in a strict order and to take account of their properties .

Question 38

Group 1 elements are

Answer 38

reactive, soft metals .Also known as alkali metals . They all have only one electron in their outer shell making them very reactive and initally all have the same properties.

Question 39

The trends for alkali metals as you go down

Answer 39

include increasing reactivity
Lower meling and boiling points
higher relative atomic mass

Question 40

alkali metals form

Answer 40

ionic compounds with non-metals

Question 41

When group 1 metals are put in water

Answer 41

they react vigarously.

Question 42

Group 7 elements are

Answer 42

known as halogens . Halogens are all non-metals with coloured vapours.

Question 43

As you go down group 7 the halogens

Answer 43

become less reactive- its harder to gain an extra electron because the outer shells further from the nucleus .
They have higher melting and boiling points
higher relative atomic mass.

Question 44

Halogens can form

Answer 44

molecular compounds and ionic bonds with metals

Question 45

Group 0 elements

Answer 45

are all inert, colourless gases. They are known as noble gases.

Question 46

Noble gases exist as

Answer 46

monatomic gases which means single atoms not bonded to each other.

Question 47

Group 0 have

Answer 47

eight electrons in their energy level apart from helium which has giving them a full outer shell.

Question 48

The boiling points of noble gases

Answer 48

increase as you move down. Due to an increase in the number of electrons in each atom leader to greater intermolecular forces.