Atomic structures

Question 1

What is a mixture?

Answer 1

When two or more elements or compounds are mixed together but aren’t chemically bonded

Question 2

What is an element?

Answer 2

A pure substance made up of only one type of atom

Question 3

What is a compound?

Answer 3

A substance that is made up of two or more atoms which are chemically bonded together

Question 4

What does soluble means?

Answer 4

When something can dissolve

Question 5

What does insoluble mean?

Answer 5

When something is unable to dissolve

Question 6

Name the subatomic particles

Answer 6

Electron
Proton
Neutron

Question 7

What does the mass tell us?

Answer 7

Protons+ neutrons

Question 8

What does the atomic number tell us?

Answer 8

Protons which is the same as electrons

Question 9

What is periodic table arranged in?

Answer 9

Atomic number (protons)

Question 10

What is an isotope?

Answer 10

A version of the same element but with a different number of neutrons

Question 11

What is the relative mass of a proton?

Answer 11

1

Question 12

What is the relative mass of a electron?

Answer 12

Very small

Question 13

What is the relative mass of a neutron?

Answer 13

1

Question 14

What is the electric charge of a proton?

Answer 14

+1

Question 15

What is the electric charge of a electron?

Answer 15

-1

Question 16

What is the electric charge of a neutron?

Answer 16

0

Question 17

When did Mendeleev organise the periodic table?

Answer 17

1869

Question 18

What did Mendeleev organise the periodic table according to?

Answer 18

To the element’s atomic mass

Question 19

How did Mendeleev group the elements?

Answer 19

Corresponding to their chemical properties

Question 20

Why did Mendeleev place the alkaline metals in one group together?

Answer 20

Because they had similar properties

Question 21

Why are transition metals placed between groups 2 and 3?

Answer 21

Because they have a similar number of electrons in their third shell

Question 22

Why did Mendeleev leave gaps?

Answer 22

For missing elements

Question 23

How created the table we use today?

Answer 23

Henry Mosely

Question 24

When did Henry Mosely produce the table we use today?

Answer 24

1914

Question 25

How did Mosely organise the elements?

Answer 25

According to their atomic number

Question 26

What did Mosely add to the table?

Answer 26

The noble gases

Question 27

Who first organised the periodic table according to their atomic mass?

Answer 27

John Newland

Question 28

When was the electron discovered and who by?

Answer 28

J.J Thompson and in 1897

Question 29

What did J.J Thompson create?

Answer 29

The plum pudding model- he imagined the atom was positively charged with electrons stuck in it

Question 30

Who tested J.J Thompson's theory and when?

Answer 30

1991 Rutherford

Question 31

How did Rutherford test Thompson's theory?

Answer 31

He fired particles at atoms however some bounced off funny not centred

Question 32

When was the proton and neutron discovered and by who?

Answer 32

By Chadwick in 1932

Question 33

What reaction would take place with the hot tungsten was surrounded by air?

Answer 33

It would react with oxygen and burn out

Question 34

What is Rn used for?

Answer 34

Radiotherapy

Question 35

What is Kr and Xe used for?

Answer 35

Lasers

Question 36

What are metals?

Answer 36

They losers because they want to react to achieve a full outer shell so they have to give away their electrons

Question 37

Name some properties of a metal

Answer 37

Good conductor of heat and electricity High density Strong solid

Question 38

Name some properties of a non metal

Answer 38

Poor conductor of heat and electricity Low density Soft Solid, liquid or gas

Question 39

What elements are the halogens?

Answer 39

Chlorine, fluorine, bromine, iodine and astatine

Question 40

What metals do the halogens react with ?

Answer 40

Alkali metals to form halide ions with a charge of -1

Question 41

What happens when you go down group 7?

Answer 41

The reactivity decreases

Question 42

Why does the reactivity of group 7 decrease as you go down?

Answer 42

As you go down the group you gain shells and for non metals to react they need to gain electrons. So it is harder to gain electrons because it is further away from the nucleus

Question 43

What happens when you go down group 1?

Answer 43

The reactivity increases

Question 44

Why does the reactivity of group 1 increase as you go down?

Answer 44

Because for metals to gain a full outer shell they lose electrons so when you go down the group the number of shells increase so the nucleus attraction is weaker. So it is easier to lose electrons

Question 45

What are the key properties of the alkali metals?

Answer 45

Low density Soft Float

Question 46

What do alkali metals react with?

Answer 46

Oxygen and hydrogen to form a hydroxide

Question 47

What is displacement?

Answer 47

When a more reactive metal displaces a less reactive metal

Question 48

What is oxidation?

Answer 48

Loss of electrons

Question 49

What is reduction?

Answer 49

Gain of electrons

Question 50

Acid + metal equals

Answer 50

Soluble salt + hydrogen

Question 51

What type of ion does all acids contain?

Answer 51

Hydrogen ions

Question 52

What happens when acids are dissolved in water?

Answer 52

They fully ionise to release H+ ions into a solution, making it strong

Question 53

Insoluble base (oxide) + acid equals

Answer 53

Soluble salt + water

Question 54

Insoluble salt (carbonate) + acid equals

Answer 54

Soluble salt + water + carbon dioxide