🧪Chemistry⚛️ year 10

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36 Terms

1

Physical change

A change in matter that does not form new substances.

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2

Examples of physical changes

Change in

  • Position

  • Shape

  • Size

  • State

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3

Chemical change/reaction

A change in matter that forms one or more new substances.

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4

Examples of chemical changes

  • release of light or sound

  • Formation of a new gas

  • Change in colour

  • Disappearance of a solid

  • Formation of a new solid

  • Change in temperature

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5

Atom

The smallest particle of an element

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6

Molecule

A group of atoms bonded together

Fixed formula, e.g. O2, H2O

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7

Chemical bond

An attractive force that holds two atoms together

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8

Mixture

A combination of substances that can be physically seperated.

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9

Element

Any of the basic substances on the periodic table, such as oxygen (O2), iron (Fe) and gold (Au).

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10

Compound

Made up of two or more different types of atoms bonded together, such as carbon dioxide (CO2) and sodium chloride (NaCl).

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11

Chemical equation

Reactants—>Products

e.g. sodium + oxygen → sodium oxide

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12

Reactants

The substances that react with each other

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13

Products

The new substances formed by a reaction

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14

The re-arrangement of atoms

  • During a chemical reaction, some of the chemical bonds between atoms are broken and new bonds are formed.

  • This re-arrangement of atoms is what produces a new substance.

  • The same elements are present after a reaction – they're just arranged in a new way.

<ul><li><p><span>During a chemical reaction, some of the chemical bonds between atoms are broken and new bonds are formed. </span></p></li><li><p><span>This re-arrangement of atoms is what produces a new substance.</span></p></li><li><p><span>The same elements are present after a reaction – they're just arranged in a new way.</span></p></li></ul><p></p>
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15

Why the two sides of a chemical equation are equal

  • Atoms cannot be created or destroyed, and the type of elements present in a chemical reaction stays the same.

  • No new elements are formed, the bonds are just rearranged in different ways, forming new substances.

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16

Metal atom

1, 2, or 3 electrons in outer shell

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17

Non-metal atom

5, 6 or 7 electrons in outer shell

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18

Lattice

Continuous arrangements of bonded atoms in regular patterns.

  • Ratio of elements, e.g. NaCl, Au

<p>Continuous arrangements of bonded atoms in regular patterns.</p><ul><li><p>Ratio of elements, e.g. NaCl, Au</p></li></ul><p></p>
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19

Why do elements bond together?

Atoms form chemical bonds to obtain full valence shells.

  • By bonding together in chemical reactions, atoms can reach a more stable state.

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20

Ions

Charged particles formed when atoms either lose or gain electrons

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21

Cations

Positively charged ions formed by the loss of electrons

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22

Anions

Negatively charged ions formed by the gain of electrons

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23

Ionic bonds

  • The transfer of electrons from one atom to another results in two ions with opposite charges. The attraction between these opposite charges is what makes an ionic bond.

  • Occurs between metals and non metals

  • Metal cations

  • Non-metal anions

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24

Predicting ionic compounds

E.g: Aluminium + Chloride

Aluminium- Metal, charge of 3+

Chloride- Non-metal, charge of 1-

This means you need three negative charges to balance out the positive charge of three.

(Al³⁺)+ (Cl⁻)+ (Cl⁻)+ (Cl⁻)

= AlCl₃

  • metals are always written before non-metals

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25

Metallic bonding

  • When metals bond with metals, they donate their valence electrons into a common pool.

  • This results in metal cations floating on a sea of delocalised electrons

  • The positively charged metal ions (cations) are held together by the attraction to this sea of delocalized electrons.

<ul><li><p>When metals bond with metals, they donate their valence electrons into a common pool.</p></li><li><p>This results in metal cations floating on a sea of delocalised electrons</p></li><li><p>The positively charged metal ions (<strong>cations</strong>) are held together by the attraction to this <strong>sea of delocalized electrons</strong>.</p></li></ul><p></p>
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26

Properties of metals explained by metallic bonding- Electrical Conductivity

Delocalised electrons can move freely through the metal- a flow of electrons is an electric current

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27

Properties of metals explained by metallic bonding- Heat Conductivity

The delocalised electrons carry thermal energy (heat) through the metal quickly and easily.

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28

Properties of metals explained by metallic bonding- Shine

Delocalised electrons move quickly so that light can reflect off all surfaces of the metal.

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29

Covalent bonding

When non-metals bond with non-metals, they share a pair of electrons between atoms.

  • Each atom contributes one or more electrons to form a shared pair.

  • This sharing allows both atoms to achieve a stable electron configuration (a full outer shell).

<p>When non-metals bond with non-metals, they share a pair of electrons between atoms.</p><ul><li><p>Each atom contributes one or more electrons to form a <strong>shared pair</strong>.</p></li><li><p>This sharing allows both atoms to achieve a <strong>stable electron configuration</strong> (a full outer shell).</p></li></ul><p></p>
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30

How to represent covalent bonding

F-F, H-H, H-O-H

<p>F-F, H-H, H-O-H</p>
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31

Bonds of common elements

H, F, Cl- one bond

O- two bonds

N- three bonds

C- four bonds

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32

Law of Conservation of Matter

  • In a chemical reaction, atoms are not created or destroyed.

  • Total number of atoms of each element remains the same before and after the reaction.

  • Atoms are just rearranged to form new substances.

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33

Unbalanced Equations

  • An equation is unbalanced if the number of atoms of each element is not the same on both sides.

Example (Unbalanced Thermite Reaction):
Fe₂O₃ + Al → Fe + Al₂O₃

  • The number of Fe and Al atoms do not match.

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34

Balancing equations

An equation is balanced when the number of each type of atom is the same on both sides.

To balance an equation:

  • Adjust the numbers in front of chemical formulas (coefficients).

Example (Balanced Thermite Reaction):
Fe₂O₃ + 2Al2Fe + Al₂O₃

<p></p><p>An equation is balanced when the number of each type of atom is the same on both sides.</p><p><strong>To balance an equation:</strong></p><ul><li><p>Adjust the numbers <strong>in front of chemical formulas</strong> (coefficients).</p></li></ul><p><strong>Example (Balanced Thermite Reaction):</strong><br><em>Fe₂O₃ + </em><strong><em>2Al</em></strong><em> → </em><strong><em>2Fe</em></strong><em> + Al₂O₃</em></p><p></p>
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35

Subscripts and coefficients in chemical equations

  • When balancing an equation, you can’t change the subscript numbers, as this shows how the molecule is naturally formed.

  • You can only adjust the coefficients, which change the number of elements or compounds in a chemical equation.

  • To find the amount of each type of atom, multiply the coefficient by the subscript

<ul><li><p>When balancing an equation, you can’t change the subscript numbers, as this shows how the molecule is naturally formed.</p></li><li><p>You can only adjust the coefficients, which change the number of elements or compounds in a chemical equation.</p></li><li><p>To find the amount of each type of atom, multiply the coefficient by the subscript</p></li></ul><p></p>
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36

How to balance equations

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