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Year 10 Science Revision (Book Section System) > Chemistry Section 1 & 2 > Flashcards

Chemistry Section 1 & 2 Flashcards

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1
Q

Define what a compound is

A

Two or more elements Chemically combined

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2
Q

Define what a mixture is

A

Two or more substances in any quantity

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3
Q

Define what relative atomic mass is

A

An average of the atomic masses of all the isotopes of an element taking into account the relative abundances/percentage of each isotope

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4
Q

How are elements arranged in the periodic table

A

In order of reactivity

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5
Q

Why do elements in the same group of the periodic table have similar chemical properties

A

They have the same number of electrons on the outer shell

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6
Q

The elements in group 0 are known as the:

A

Noble gasses

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7
Q

The elements in group 1 are known as the:

A

Alkali Metals

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8
Q

The elements in group 7 are known as the:

A

Halogens

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9
Q

What is an atom

A

The smallest part of an element that can exist

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10
Q

What is on the left and right of a chemical equation?

A

Left: reactants Right: products

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11
Q

How is an element different to a compound

A

A compound

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12
Q

What is the equation for Neutrons?

A

Number of neutrons = mass number - atomic number

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13
Q

How are the groups arranged?

A

By number of electrons on the outer shell: 1 electron = group 1

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14
Q

Do melting and boiling points increase or decrease down the alkali metals?

A

Decrease

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15
Q

What does aqueous mean (aq)

A

Dissolved in water

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16
Q

What are the three types of strong chemical bonds

A

Ionic bonds, covalent bonds, metallic bonds

17
Q

Atoms that have gained or lost electrons are called:

A

Ions

18
Q

Ionic bonds occur between:

A

Positive and negative ions

19
Q

Ions have a:

A

complete outer shell of electrons

20
Q

Ionic bonding involves a transfer of electrons from:

A

Metal atoms to non-metal atoms

21
Q

The ionic bond is a strong ——- force of attraction between the positive metal ion and the negative non-metal ion

A

Electrostatic

22
Q

Describe what happens when two atoms of sodium react with one molecule of chlorine

A

Sodium (Group1)
Chlorine (Group7) has 2 atoms in a molecule.
The two atoms of sodium each give one electron from their outer shells, completing the 7/8 outer shells of the chlorine.
All 4 atoms now have 8 electrons in their outer shells.
The atoms become ions, Na+ and Cl-, the compound formed is sodium chloride, NaCl

23
Q

A covalent bond is a:

A

shared pair of electrons between atoms.

24
Q

covalent bonds occur in:

A

Non metallic elements, eg oxygen
Compounds of non metals, eg sulfur dioxide

25
Q

Small molecules have weak ——– forces of attraction

A

Intermolecular

26
Q

Substances that consist of small molecules usually have low ————————–

A

Melting and boiling points

27
Q

All the atoms in giant covalent structures are linked by ———————-

A

Strong covalent bonds

28
Q

Why does Hydrogen chloride have a low boiling point

A

Although there is a strong covalent bond within the molecule, there are only weak intermolecular forces between molecules

29
Q

Describe the structure of diamond

A

-It has a giant rigid covalent structure
-Each carbon atom forms four strong covalent bonds with other carbon atoms
-All the strong covalent bonds mean that it is a very hard substance with a very high melting point

29
Q

Explain how graphite can conduct electricity

A

One electron from each carbon atom in graphite is delocalised, these delocalised electrons allow graphite to conduct heat and electricity

29
Q

How does the size of a small molecule affect the strength of the intermolecular forces between molecules

A

The bigger the molecule, the larger the intermolecular forces

29
Q

Alkanes contain atoms of which two elements

A

Carbon and Hydrogen

29
Q

Which is weak in small molecules, intermolecular bonds or covalent bonds

A

Intermolecular

29
Q

Explain why diamond is hard

A

Because there are strong covalent bonds in between all the carbon atoms

29
Q

Explain why graphite can conduct electricity

A

Because there are delocalised electrons between the layers which can carry charge

30
Q

What is graphene

A

A single layer of graphite

30
Q

State some properties of graphene

A

It is very strong, a good thermal and electrical conductor and nearly transparent

31
Q

What is a metallic bond

A

A metallic bond is the attraction between the positive ions and the delocalised negatively charged electrons

31
Q

Why is copper a good material for water pipes

A

Because it is unreactive and is easily shaped

Year 10 Science Revision (Book Section System) (8 decks)

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