C1- Atomic structure and the periodic table

Question 1

Define isotope

Answer 1

Different forms of the same element which have the same number of protons but a different number of neutrons.

Question 2

Define element

Answer 2

An element is a substance made up of atoms that all have the same number of protons in their nucleus.

Question 3

To find the number of neutrons in an atom you?

Answer 3

Subtract the atomic number from the mass number.

Question 4

Which number is the mass number and what does it tell you?

Answer 4

The top number
It tells you the total number of protons and neutrons in the atom.

Question 5

Which number is the atomic number and what does it tell you?

Answer 5

The bottom number
It tells you the number of protons.

Question 6

What is an ion?

Answer 6

An atom or group of atoms that has lost or gained electrons.

Question 7

Why do ions have an overall charge?

Answer 7

The number of protons do not equal the number of electrons.

Question 8

Why do atoms not have an overall charge?

Answer 8

They have the same number of protons and electrons so the charges cancel out

Question 9

Number of protons in an atom is equal to?

Answer 9

The number of electrons.

Question 10

The volume of the whats orbit determines the size of the atom?

Answer 10

Electrons

Question 11

Electrons move around the nucleus in?

Answer 11

Shells

Question 12

State the relative mass of protons, neutrons and electrons

Answer 12

Protons= 1
Neutrons= 1
Electrons= Almost 0

Question 13

State the charge of protons, neutrons and electrons

Answer 13

Protons= +1
Neutrons= 0
Electrons= -1

Question 14

Where is most of the mass of the atom concentrated?

Answer 14

The nucleus

Question 15

What is the radius of the nucleus?

Answer 15

1x10^-14m

Question 16

What is the overall charge of the nucleus?

Answer 16

Protons + Neutrons = Positive charge

Question 17

What is the radius of the atom?

Answer 17

0.1 nanometres
(1x10^-10m)

Question 18

Isotopes have the same ________ number but different _______ numbers.

Answer 18

Atomic
Mass

Question 19

How are compounds formed?

Answer 19

When elements react atoms combine with other atoms to from compounds.

Question 20

Define Compound

Answer 20

Substances formed by two or more elements, the atoms of each are in fixed proportions throughout the compound and they’re held together by chemical bonds.

Question 21

What happens when a bond is made?

Answer 21

Involves giving atoms away and taking or sharing electrons.

Question 22

How can you serrate the original elements of a compound?

Answer 22

Through a chemical reaction.

Question 23

What is an ionic compound formed from?

Answer 23

One formed from a metal and a non metal.

Question 24

The metal ion in the compound ______ electrons to form______ ions and the non metal does the opposite.

Answer 24

Loses
Positive

Question 25

What is ionic bonding?

Answer 25

The opposite charges of the ions causes a strong attraction.

Question 26

What does a compound made of non metals consist of?

Answer 26

Molecules

Question 27

What type of bonding is in a molecular compound?

Answer 27

Covalent bonding

Question 28

What is covalent bonding?

Answer 28

An atom sharing an electron with another atom

Question 29

Properties of a compound are different or the same as the original elements

Answer 29

Usually completely different

Question 30

What shows the elements in a compound

Answer 30

A formula such as CO2

Question 31

Define nucleus

Answer 31

Contains protons and neutrons and nearly the whole mass of the atom is concentrated in the nucleus.

Question 32

What is a mixture?

Answer 32

Elements or compounds with no chemical bond between them, that can be separated using physical methods. It does not form new substances.

Question 33

List 5 physical methods of separating mixtures

Answer 33

Filtration Crystallisation Simple distillation Fractional distillation Chromatography

Question 34

How did John Dalton describe atoms?

Answer 34

Solid spheres of different elements

Question 35

How did JJ Thompson describe atoms?

Answer 35

Plum pudding model Ball of positive charge with negatively charged electrons embedded in it

Question 36

How did Ernest Rutherford describe atoms?

Answer 36

Nuclear model A tiny positively charged nucleus at the centre where the mass is concentrated. A cloud of negative electrons surround the nucleus. It is mostly empty space.

Question 37

Why was Rutherford wrong?

Answer 37

The cloud of negative electrons would be attracted and the atom would collapse.

Question 38

How did Neil's Bohr describe atoms?

Answer 38

Electrons orbit in shells at a fixed distance from the nucleus.

Question 39

Who discovered protons?

Answer 39

Rutherford

Question 40

Who discovered neutrons?

Answer 40

James Chadwick

Question 41

What was the order of discovery of parts of the atom?

Answer 41

Atom Electrons Nucleus Protons Neutrons

Question 42

What was the order of people atom discovery?

Answer 42

Leviticus John Dalton JJ Thompson Ernest Rutherford Neil's Bohr James Chadwick

Question 43

How do you know the electronic structure of an element?

Answer 43

Atomic number = protons Protons = electrons

Question 44

How was the periodic table arranged in early 1800s?

Answer 44

Their physical and chemical properties Their relative atomic mass

Question 45

What is relative atomic mass?

Answer 45

The average mass of one atom of an element

Question 46

Who left gaps and predicted elements in the periodic table?

Answer 46

Dmitri Mendeleev

Question 47

When did Dmitri make his table?

Answer 47

1869

Question 48

How did Mendeleev order his table?

Answer 48

Mostly in order of atomic mass but switched order if elements had similar properties.

Question 49

How is the modern periodic table arranged?

Answer 49

Increasing atomic (proton) number

Question 50

Which side are metals found?

Answer 50

Left

Question 51

What does the group number tell you?

Answer 51

The number of electrons in the outer shell

Question 52

Properties of metals

Answer 52

Strong Malleable Good conductors of heat and electricity High boiling points and melting points

Question 53

Why are metals more likely to form positive ions when they react?

Answer 53

They don't have many electrons to lose and they need less energy to lose electrons as they have a weaker attraction.

Question 54

Properties of non metals

Answer 54

Dull looking and brittle Some are not solids at room temperature Don't conduct electricity They often have a lower density

Question 55

What are transition metals?

Answer 55

Typical metals with some additional properties

Question 56

What are the properties of transition metals?

Answer 56

Can have more than one ion Often coloured metal ions Good catalysts

Question 57

Properties of group 1 elements

Answer 57

Very reactive Soft Low density Alkali metals

Question 58

What is the trend of alkali metals as you go down group one?

Answer 58

Increasing reactivity Lower melting point Lower boiling point Higher relative atomic mass

Question 59

What do alkali metals and non metals form?

Answer 59

Ionic compounds

Question 60

How do group 1 metals react with water?

Answer 60

React vigorously to produce hydrogen gas and metal hydroxides, compounds that dissolve in water to produce alkaline solutions

Question 61

How does potassium react with water?

Answer 61

Ignites hydrogen

Question 62

How do group 1 metals react with chlorine?

Answer 62

React vigorously when heated in chlorine gas to form white metal chloride salts

Question 63

How do group 1 metals react with oxygen?

Answer 63

React to form a metal oxide Lithium forms lithium oxide Sodium forms a mixture of sodium oxide and peroxide Potassium reacts to form a mixture of potassium peroxide and superoxide

Question 64

What are the properties of group 7 elements?

Answer 64

Halogens Non metals Coloured vapours Molecules or pairs of atoms

Question 65

Properties of fluorine

Answer 65

Very reactive Poisonous Yellow Gas

Question 66

Properties of chlorine

Answer 66

Fairly reactive Poisonous Dense Green Gas

Question 67

Properties of bromine

Answer 67

Dense Poisonous Red brown Volatile Liquid

Question 68

Properties of iodine

Answer 68

Dark grey Crystalline Solid OR Purple Vapour

Question 69

What happens when you go down group 7?

Answer 69

The halogens become less reactive Have higher melting and boiling points Have higher relative atomic masses

Question 70

What do halogens and non metals form?

Answer 70

Molecular compounds Simple molecular structures

Question 71

What do halogens and metals form?

Answer 71

Ionic bonds Ionic structured compounds

Question 72

When does a displacement reaction occur?

Answer 72

Between a more reactive halogen and the salt of a less reactive one

Question 73

Properties of group 0 elements

Answer 73

Noble gases Inert Colourless at room temperature Full outer shell Monatomic gases or single atoms not bonded to each other Non flammable

Question 74

What happens to group 0 elements as you go down the table?

Answer 74

The boiling points increase The relative atomic masses increase