C1 Atomic structure and periodic table

Question 1

define element

Answer 1

made up of the same type of atom and cannot be chemically split up further

Question 2

define compound

Answer 2

two or more different atoms that are chemically bonded

Question 3

define mixture

Answer 3

two or more atoms that are not chemically bonded

Question 4

define empirical formula

Answer 4

The simplest ratio of atoms of each element in a compound

Question 4

define empirical formula

Answer 4

The simplest ratio of atoms of each element in a compound

Question 5

how do you calculate the empirical formula?

Answer 5

• count up number of each type of ion
• divide by the smaller number
• round to the nearest whole number

Question 6

define solute

Answer 6

the name of what you dissolve

Question 7

define solvent

Answer 7

the name of what you dissolve the solute in

Question 8

define solution

Answer 8

the outcome of dissolving the solute in the solvent

Question 9

define soluble

Answer 9

a name you give to a substance that can be dissolved

Question 10

define insoluble

Answer 10

a name you give to a substance that cannot be dissolved

Question 11

define solubility

Answer 11

the amount of solute that can be dissolved in 100g of solvent

Question 12

through which experiment did John Thompson discover electrons mainly?

Answer 12

The Vaccum Tube

Question 13

what did the experiment The Vacuum Tube show?

Answer 13

showed negatively charged particles flowing through an electrical current

Question 14

what misconception did John Thompson think about electrons after the Vacuum Tube experiment?

Answer 14

he thought that electrons were part of the atom because they were much smaller and alike

Question 15

what model of the atom did John Thompson make after the Vacuum Tube experiment?

Answer 15

the plum pudding model

Question 16

describe the plum pudding model

Answer 16

had an area of positive space and had negative electrons randomly spotted in the middle

Question 17

what experiment did Ernest Rutherford do?

Answer 17

the alpha particle scattering experiment

Question 18

what was the alpha scattering experiment?

Answer 18

fired alpha particles (He2+ ions) at a piece of gold foil

Question 19

what 4 things did Ernest Rutherford learn about the atom from the alpha particle scattering experiment?

Answer 19

• there is a positive nucleus in the middle
• electrons are around the nucleus
• the mass of the atom is concentrated at the middle
• most of the atom is space

Question 20

how did Ernest know that there is a positive nucleus in the middle from the a.p.s experiment?

Answer 20

the particles were reflected/refracted by this and re-directed

Question 21

how did Ernest know that the mass of the atom is concentrated in the middle from the a.p.s experiment?

Answer 21

some of the particles were deflected and some of them went straight through

Question 22

describe what changes Bohr made to the nuclear model

Answer 22

he put electrons set distance from the nucleus and they are orbiting it, these are called shells/energy levels

Question 23

describe 4 differences between the nuclear model and plum pudding model?

Answer 23

-plum pudding model has no nucleus
-in the ppm the mass was evenly distributed but in the nm its concentrated in the middle
-most of the nm is space but in the ppm there are no spaces
-in the ppm electrons are randomly plotted around but in the nm they are around the positive nucleus

Question 24

why are lithium and sodium both in group 1?

Answer 24

they both have 1 electron in their outer shell

Question 25

explain why sodium is more reactive than lithium

Answer 25

-sodium has more shells/its a bigger atom -weaker force of attraction between outer electron and positive nucleus -makes the outer electron easier to lose

Question 26

give 2 observations you can see when potassium is added to water

Answer 26

-fizzing with bubbles -the potassium floats on the water

Question 27

explain why sodium oxide has a high melting point

Answer 27

- sodium oxide has a giant ionic structure - have strong electrostatic forces of attraction between oppositely charged ions - requires a lot of energy to break

Question 28

give one limitation to using a dot and cross diagrams

Answer 28

doesn't show the shape/ only two diminsional

Question 29

give one limitation to using a dot and cross diagrams

Answer 29

doesn't show the shape/ only two dimensional

Question 30

define isotope

Answer 30

an atom of the same element that has the same number of protons but a different number of neutrons

Question 31

what is the formula to find the relative atomic mass of an element with different isotopes?

Answer 31

(mass number x percentage) of isotope 1 +(mass number x percentage) of isotope 2 / 100

Question 32

give the charge of a proton

Answer 32

positive charge +1

Question 33

give the charge of a neutron

Answer 33

neutral charge 0

Question 34

give the charge of a electron

Answer 34

negative charge -1

Question 35

what is the relative mass of a proton?

Answer 35

1 m u (atomic mass units)

Question 36

what is the relative mass of a neutron?

Answer 36

1 m u (atomic mass units)

Question 37

what is the relative mass of a electron?

Answer 37

1/2000 m u (atomic mass units)

Question 38

how are the elements in the parodic table arranged?

Answer 38

atomic number / number of protons

Question 39

how are elements with similar properties place in the periodic table?

Answer 39

they are placed in groups

Question 40

how did Newlands order his perodic table?

Answer 40

by their atomic weight

Question 41

what were the 'groups' Newlands ordered his table called?

Answer 41

octaves

Question 42

how did Mendeleev order his periodic table?

Answer 42

by their atomic weight

Question 43

what are the 2 main differences between Newlands and Mendeleev's periodic table?

Answer 43

1) M predicted elements that hadn't been discovered yet and left gaps for these undiscovered elements 2) M altered the strict order of atomic weight so their properties could match

Question 44

why are the noble gases unreactive?

Answer 44

because they already have full outer shells

Question 45

why was Mendeleev's table accepted?

Answer 45

elements he predicted were discovered and their properties matched his predictions

Question 46

State two key things that Mendeleev did that no one had done before that made his Table work?

Answer 46

- left gaps for elements he believed were yet to be discovered - changed from weight order for some elements to put them in groups with elements with similar properties

Question 47

Describe metallic bonding

Answer 47

attraction between nucleus of metal atoms in a lattice to the cloud of delocalised outer shell electrons

Question 48

Explain why sodium is soft

Answer 48

atoms all the same sizecan slide over each other while maintaining metallic bonding

Question 49

Explain why bromine has a low boiling point

Answer 49

weak forces between molecules

Question 50

Sodium reacts with bromine to form sodium bromide. Explain why this reaction takes place in terms of electrons

Answer 50

electrons transferred from sodium atoms to bromine atomsin order for all atoms toget stable electron structures of group 0 atoms

Question 51

Explain why sodium bromide has a high melting point

Answer 51

strong attraction between positive and negative ions

Question 52

give 2 similarities in physical properties between group 1 metals and transition metals

Answer 52

*conduct heat *conduct electricity *malleable *ductile *shiny when polished

Question 53

give 2 similarities in chemical properties between group 1 metals and transition metals

Answer 53

*react with non-metals to form ionic compounds *form basic oxides

Question 54

give 2 differences in chemical properties between group 1 metals and transition metals

Answer 54

*K is (much) more reactive *Cu forms ions with different charges, K only forms 1+ ions *Cu forms coloured compounds but K forms white compounds

Question 55

give 2 differneces in physical properties between group 1 metals and transition metals

Answer 55

*Cu has (much) higher melting point *Cu has (much) higher density

Question 56

What method would you use to separate ethanol from a solution of sugar in ethanol

Answer 56

distillation

Question 57

What method would you use to separate ethanol from a mixture of water and ethanol (they are miscible liquids)

Answer 57

fractional distillation

Question 58

What method would you use to separate water from a mixture of hexane and water (they are immiscible liquids)

Answer 58

separating funnel

Question 59

What method would you use to separate iron filings from a mixture of iron filings with water

Answer 59

filtration

Question 60

what can we separate?

Answer 60

mixtures

Question 61

what does chromatography separate?

Answer 61

solid from another soluble solid

Question 62

what does filtration separate?

Answer 62

insoluble solids from a solution

Question 63

what does distillation separate?

Answer 63

soluble solute from a solution

Question 64

what does evaporations separate?

Answer 64

soluble solute from a solution

Question 65

what is the difference between the reason why you sometimes use evaporation to separate and distillation to separate?

Answer 65

sometime you need to collect the solvent itself instead of it just evaporating off

Question 66

how is simple distillation different to fractional distillation?

Answer 66

SD separates substances with greater difference between boiling points FD separates substances with boiling points that are closer to each other

Question 67

Lithium, sodium and potassium are all in group 1 of the periodic table. Which of these has the lowest boiling point?

Answer 67

The melting points of the group 1 metals decrease as you go down the group.