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3s and 4s Clevedon Science > C4 Part 1 > Flashcards

C4 Part 1 Flashcards

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1
Q

Describe the structure of an atom.

A

Every atom is made of a nucleus consisting of protons and neutrons. The nucleus is surrounded by electrons.

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2
Q

What is the charge of an electron?

A

-1

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3
Q

What is the mass of an electron?

A

0

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4
Q

What is the charge of a proton?

A

+1

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5
Q

What is the mass of a proton?

A

1

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6
Q

What is the charge of a neutron?

A

0

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7
Q

What is the mass of a neutron?

A

1

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8
Q

Why do atoms have a neutral charge?

A

There are the same number of protons (positive charges) as electrons (negative charges)

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9
Q

What is an isotope?

A

Isotopes are atoms of the same element but with different mass numbers. The mass numbers are different because they have different numbers of neutrons in the nucleus.

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10
Q

What is the mass of an atom?

A

10-23g

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11
Q

What is the radius of an atom?

A

10-10m

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12
Q

Describe how the elements in the periodic table are arranged.

A

They are arranged in ascending order of atomic number.

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13
Q

What is the atomic number?

A

Atomic number is the number of protons in an atom.

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14
Q

What is the atomic number of carbon?

A

6

Carbon therefore has 6 protons and 6 electrons

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15
Q

What does the mass number of an atom tell you?

A

The mass number is the total number of protons and neutrons in an atom.

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16
Q

What is the mass number of fluorine?

A

19

Fluorine has 19 protons and neutrons

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17
Q

How are electrons arranged in an atom?

A

2 electrons can go in the first shell. The subsequent shells fill up by 8 electrons.

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18
Q

What is the elctronic structure of potassium?

A

Potassium has 19 electrons.

The electronic structure is 2,8,8,1

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19
Q

How did John Dalton describe atoms in the 19th century?

A

John Dalton thought that atoms were solid spheres and that these solid spheres made up the different elements.

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20
Q

What was JJ Thompson’s theory of atomic structure in 1897?

A

“Plum pudding model”

Thompson thought that atoms must contain smaller negatively charged particles called electrons which were found throughout the atom.

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21
Q

What experiments did Rutherford carry out in 1909?

What did he deduce about the structure of an atom?

A

Rutherford fired positively charged particles at a thin sheet of gold. Most particles passed straight through the gold.

Rutherford thought that atoms must have a tiny positively charged nucleus surrounded by a “cloud” of negative electrons.

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22
Q

Describe Bohr’s model of the atom.

A

Electrons exist in fixed orbits around the nucleus.

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23
Q

What are vertical columns in the periodic table known as?

A

Groups

24
Q

What do all elements in group 1 have in common?

A

They all have 1 electron in their outer shell.

25
Q

What does the group number tell you about an atom?

A

It tells you how many electrons are in the outer shell.

For example atoms in group 1 have 1 electron in the outer shell and atoms in group 7 have 7 electrons in the outre shell.

26
Q

What are rows in the periodic table known as?

A

Periods

27
Q

How did Dobereiner organise the elements in 1828?

A

He put the elements in to groups of three called triads based on their chemical properties.

28
Q

How did Newlands arrange the elements in 1894?

A

He arranged them in sets of 8 called Newland’s Octaves. Every eigth element had similar properties.

29
Q

How did Mebdeleev arrange the elements in 1869?

A

He put elements in order of atomic mass and left gaps so that elements were grouped with similar properties.

30
Q

What is an ion?

A

An ion is an atom that has lost or gained electrons to become charged.

31
Q

How do metals form positive ions?

A

Metals lose electrons

32
Q

What is an ionic bond?

A

Ionic bonds are formed between metals and non-metals.

Metals lose elctrons to become positively charged. Non metals gain electrons to become negatively charged. These ions are attracted to each other as they have opposite charges.

33
Q

Draw a dot and cross diagram to show the ionic bonding between Sodium (Na) and Chlorine (Cl) to form Sodium Chloride (NaCl)

A
34
Q

What type of structure do ionic compounds form?

A

Giant ionic lattices

Ions form a closely packed regular lattice arrangmenent

35
Q

Give three properties of giant ionic compounds such as NaCl and MgO. Explain these properties.

A
  1. Do not conduct electricity when solid because the ions cannot move.
  2. High melting points and boiling points because the forces of attractin between the oppositely charged ions are very strong.
  3. Conduct electricity when molten or dissolved because the ions can move
36
Q

How do non-metals bond?

A

They form covalent bonds by sharing electrons.

37
Q

Draw a dot and cross diagram to show the covalent bonding in hydrogen gas, H2

A
38
Q

Draw a dot and cross diagram to show the covalent bonding in chlorine gas, Cl2.

A
39
Q

Draw a dot and cross diagram to show the covalent bonding in methane, CH4.

A
40
Q

Draw a dot and cross diagram to show the covalent bonding in water, H2O.

A
41
Q

Draw a dot and cross diagram to show the covalent bonding in carbon dioxide, CO2.

A
42
Q

What kind of structure do substances formed by covalent bonds form?

A

Simple molecular structures

43
Q

Why do simple molecular substances have low melting and boiling points?

A

The intermolecular forces between the molecules are weak.

44
Q

What are the Group 1 metals commonly known as?

A

Alkali Metals

45
Q

What happens to the reactivity of group 1 metals as you go down the group?

A

Reactivity increases.

The outer electron becomes further away from the positive nucleus and is more easily lost.

46
Q

Why are the alkali metals stored in oil?

A

They are highly reactive and react with oxygen and water.

47
Q

Give 3 physical properties of the alkali metals.

A
  1. Low melting and boiling point
  2. Low density
  3. Very soft - they can be cut with a knife
48
Q

What is the process of losing electrons known as?

A

Oxidation

49
Q

What is produced when an alkali metal reacts with water?

A

Metal hydroxide and hydrogen gas

50
Q

Write the balalnced symbol equation for the reaction of lithium with water.

A

2Li + 2H2O ——> 2LiOH + H2

51
Q

Write the balanced symbol equation for the reaction of sodium with water.

A

2Na + 2H2O ——> 2NaOH + H2

52
Q

What colour flame does lithium give in a flame test?

A

Red

53
Q

What colour flame does sodium give in a flame test?

A

Yellow / Orange

54
Q

What colour flame does potassium give in a flame test?

A

Lilac

55
Q

Describe the method used for a flame test.

A
  1. Dip a wire loop i nhydrochloric acid to clean and moisten it.
  2. Put the loop into the sample powder to be tested.
  3. Place the end of the loop in a blue bunsen flame.

3s and 4s Clevedon Science (9 decks)

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