C1- Atomic Structure And The Periodic Table

Question 1

What do atoms contain

Answer 1

Protons, neutrons and electrons

Question 2

Nucleus of an atom

Answer 2

Contains protons and neutrons has positive charge due to protons

Question 3

Electrons

Answer 3

Move around nucleus in electrons shells, negatively charged, have virtually no mass

Question 4

Protons

Answer 4

Positively charged, relative mass 1, euqals number of elctrons, number of protons is atomic number

Question 5

Atoms charge

Answer 5

Nuetral, same number of protons as electrons

Question 6

Mass number of element

Answer 6

Total number of protons and neutrons

Question 7

Isotopes

Answer 7

Different forms of the same element, same number of protons but different number of neutrons

Question 8

Relative atomic mass

Answer 8

Relative atomic mass= sum of (isotope abundance x isotope mass number) divided by sum of abudance of all the isotopes

Question 9

Compounds

Answer 9

Formed when two or more elements are chemically combined

Question 10

Mixtures

Answer 10

Unlike compounds easily separated, two or more elements mixed together but no chemically combined eg. Air

Question 11

Properties of mixtures

Answer 11

A mixture of the properties of the separate parts- chemical properties of a substance aren’t affected by it being part of a mixture

Question 12

Paper chromatography method

Answer 12

1. Draw a line near bottom of filter paper using a pencil
2. Add a spot of ink to line and place in beaker of solvent
3. Make sure ink isn’t touching the solvent
4. Place a lid on top of the contsiner to stop solvent evaporating
5. Solvent seeps up paper carrying ink
6. Each dye will move up paper at different rates
7. If any dyes are insoluble they will stay on baseline
8. When solvent has nearly reached top of papertake paper out and leave to dry

Question 13

Filtration

Answer 13

Seperates insoluble solids from liquids

Question 14

Two ways to separate soluble solids from solutions

Answer 14

Evaporation, crystallisation

Question 15

Evaporation method

Answer 15

1. Pour solution into evaporating dish
2. Slowly heat solution to evaporate and the solution will get more concentrated snd crystals form
3. Keep heating the evaporating dish until all you have left are dry crystals

Question 16

Crystallisation

Answer 16

1. Pour solution into an evaporating dish and gently heat solution
2. Once crystals start to form remove dish from heat and leave to cool
3. The salt should start to form crystals as it becomes insoluble in the cold, highly concentrated
4. Filter crystals out of solution and leave them in a warm place to dry

Question 17

Simple distillation

Answer 17

Seperates liquid from solution

Question 18

Simple distillation method

Answer 18

1. Part of solution that has the lowest boiling point evaporates first
2. Vapour is then cooled, condenses and is collected
3. The rest of solution is left in flask

Question 19

Issue with simple distillation

Answer 19

Can only separate things with very different boiling points

Question 20

Fractional distillation

Answer 20

Separtes mixture of liquids with similar boiling points

Question 21

Fractional distillation method

Answer 21

1. Put mixture in flask and put fractional column on top and heat it
2. Different liquids will have different boiling point
3. Liquid with lowest boiling point evaporates first. When the temperature matches the boiling point of thie liquid, it will reach the top of the column
4. Liquids with higher boiling points may start to evaporate. But the column is cooler towards the top. So they will only get part of the way up before condensing and running back down towards the flask
5. When the first liquid has been collected, you raise the tempersture until the next one reaches the top

Question 22

John dalton

Answer 22

At start of 19th centruy Dalton described atoms as solid spheres and said that different spheres were made up the different elements

Question 23

Jj thomson

Answer 23

1808 concluded from his experiments that atoms weren’t solid spheres. His measurements of charge and mass showed that an atom must contain even smaller negatively charged particles- electrons

Question 24

Plum pudding model

Answer 24

Showed atom as a ball of positive charge with electrons stuck in it

Question 25

Alpha particle- rutherford

Answer 25

Fired positively charged alpha particles at a thin sheet of gold. Most particles went straight through, some deflected and a smaller number deflected backwards

Question 26

Rutherfords nuclear model of an atom

Answer 26

Tiny, positively charged nucleus where mass is most concentrated with cloud of electrons surrounding it so most the atom is empty space

Question 27

Bohr’s nuclear model

Answer 27

Suggested electrons were contained in fixed shells and each sheels is a fixed distsnce from the nucleus

Question 28

Electronic shell rules

Answer 28

Atoms with full electronic shells are less reactive eg group 0 (noble gases)

Question 29

Groups of periodic table

Answer 29

Vertical columns with elements of similsr properties

Question 30

Rows of periodic table

Answer 30

Called periods and each period represents another full shell of electrons

Question 31

Metals

Answer 31

From positive ions when they react

Question 32

Non metals

Answer 32

Generaly don’t form positive ions when they react

Question 33

How electronic structure of atoms affect how they react

Answer 33

Atoms form a full oiter shell by losing, gaining or sharing electrons. Metals are to the left of periodic table and metal’s outer electrons which are a long way from nucleus have a weaker attraction

Question 34

Metal properties

Answer 34

Hard to break but malleable, great heat condcutor and electricity, high boiling and melting points

Question 35

Non-metals

Answer 35

More brittle, aren’t always solid, don’t generally conduct electricity and often have lower density

Question 36

Group 1 elements properties

Answer 36

Highly reactive, soft, low density

Question 37

Group 1 metal trends

Answer 37

Increase reactivity, lower melting and boiling points, higher relative atomic mass,

Question 38

Reaction of alkali metals with water

Answer 38

Vigorous , more reactive as you go down group, float around surface fizzing furiously. Produce hydrogen and for potassium and below enough energy produced to ignite hydrogen

Question 39

Group 7 elements- the halogens

Answer 39

As you go down less reactive (harder to gain an extra electron as shell is further from nucelus), high melting and boiling point, higher relatives atomic masses, share electrons via covalent bonding

Question 40

Displacement

Answer 40

When a more reactive element displaces a less reactive element from a compound that contains the less reactive element

Question 41

Group 0 elements- noble gases

Answer 41

Full outer shell, they don’t react much at all, non-flammable, boiling point increase as you move down

Question 42

Why does boiling point increase

Answer 42

Increase in number of electrons in each atom lead to greater intermolecular forces