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Chemistry Year 8 > Untitled Deck > Flashcards

Untitled Deck Flashcards

1
Q

What is matter?

A

Anything that has mass and takes up space.

Matter is made up of tiny particles called atoms.

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2
Q

What is an atom?

A

The smallest unit of an element that retains the chemical properties of that element.

It consists of a nucleus containing protons and neutrons, surrounded by electrons.

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3
Q

What is the composition of substances?

A

All substances are composed of atoms. In elements, all atoms are the same, whereas in compounds, different types of atoms are chemically bonded together in fixed ratios.

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4
Q

Who proposed that matter is made up of tiny, indivisible particles called ‘atomos’?

A

Democritus (5th Century BCE)

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5
Q

What did John Dalton introduce in 1803?

A

The atomic theory, stating that atoms are indivisible, different elements have different atoms, and atoms combine in fixed ratios.

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6
Q

What did J.J. Thomson discover in 1897?

A

The electron and proposed the ‘plum pudding model.’

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7
Q

What significant experiment did Ernest Rutherford conduct in 1911?

A

The gold foil experiment, leading to the discovery of the nucleus.

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8
Q

What model did Niels Bohr propose in 1913?

A

That electrons orbit the nucleus in fixed energy levels (shells).

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9
Q

What did James Chadwick discover in 1932?

A

The neutron, explaining atomic mass.

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10
Q

What is the modern quantum model of the atom?

A

Electrons exist in probability clouds called orbitals rather than fixed orbits.

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11
Q

What are the three main subatomic particles of an atom?

A
  • Protons (positively charged, found in the nucleus)
  • Neutrons (neutral charge, found in the nucleus)
  • Electrons (negatively charged, orbiting the nucleus in energy levels)
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12
Q

What is the charge of a proton?

A

+1

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13
Q

What is the charge of a neutron?

A

0

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14
Q

What is the charge of an electron?

A

-1

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15
Q

Why are atoms overall neutrally charged?

A

The number of positively charged protons equals the number of negatively charged electrons.

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16
Q

What happens when the balance of protons and electrons is disrupted?

A

The atom becomes an ion.

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17
Q

List the elements in Group 1 (Alkali Metals).

A
  • Lithium (Li)
  • Sodium (Na)
  • Potassium (K)
  • Rubidium (Rb)
  • Cesium (Cs)
  • Francium (Fr)
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18
Q

What are the properties of Alkali Metals?

A
  • Extremely reactive, especially with water
  • Soft metals that can be cut with a knife
  • Low density
  • Stored in oil to prevent reactions with air/water
  • React with water to form alkaline solutions and hydrogen gas
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19
Q

What is the reactivity trend of Alkali Metals?

A

Increases down the group; Francium is the most reactive.

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20
Q

What is an example reaction involving sodium and water?

A

2Na + 2H₂O → 2NaOH + H₂

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21
Q

List the elements in Group 2 (Alkaline Earth Metals).

A
  • Beryllium (Be)
  • Magnesium (Mg)
  • Calcium (Ca)
  • Strontium (Sr)
  • Barium (Ba)
  • Radium (Ra)
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22
Q

What are the properties of Alkaline Earth Metals?

A
  • Less reactive than alkali metals
  • Harder and denser
  • React with water but not as violently
  • Good conductors of electricity
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23
Q

What is an example reaction involving calcium and water?

A

Ca + 2H₂O → Ca(OH)₂ + H₂

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24
Q

List the elements in Group 17 (Halogens).

A
  • Fluorine (F)
  • Chlorine (Cl)
  • Bromine (Br)
  • Iodine (I)
  • Astatine (At)
  • Tennessine (Ts)
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25
Q

What are the properties of Halogens?

A
  • Highly reactive nonmetals
  • Exist as diatomic molecules
  • Toxic in high concentrations
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26
Q

What is the reactivity trend of Halogens?

A

Decreases down the group; Fluorine is the most reactive.

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27
Q

What is an example reaction involving sodium and chlorine?

A

2Na + Cl₂ → 2NaCl

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28
Q

List the elements in Group 18 (Noble Gases).

A
  • Helium (He)
  • Neon (Ne)
  • Argon (Ar)
  • Krypton (Kr)
  • Xenon (Xe)
  • Radon (Rn)
  • Oganesson (Og)
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29
Q

What are the properties of Noble Gases?

A
  • Inert due to full outer electron shells
  • Colorless, odorless gases
  • Low boiling points
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30
Q

What is the common use of Helium?

A

Balloons and blimps.

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31
Q

What is the common use of Neon?

A

Neon signs.

32
Q

What is the common use of Argon?

A

Light bulbs (prevents filament burning).

33
Q

What is the chemical formula for methane?

34
Q

What is the chemical formula for carbon dioxide?

35
Q

What is the chemical formula for carbon monoxide?

36
Q

What is the chemical formula for ammonia?

37
Q

What is the chemical formula for water?

38
Q

What is the chemical formula for glucose?

A

C₆H₁₂O₆

39
Q

What is the chemical formula for sodium chloride?

40
Q

What makes atoms different for each element?

A

Each element has a unique number of protons, neutrons, and electrons.

41
Q

How is the Periodic Table organized?

A

By Groups (columns) and Periods (rows).

42
Q

What do Groups in the Periodic Table represent?

A

Elements with similar chemical properties.

43
Q

What do Periods in the Periodic Table represent?

A

Elements with increasing atomic numbers.

44
Q

How can elements be located on the periodic table?

A

By name or symbol.

45
Q

What is the unique symbol for Hydrogen?

46
Q

What is the unique symbol for Oxygen?

47
Q

Where are metals located on the Periodic Table?

A

On the left side.

48
Q

Where are non-metals located on the Periodic Table?

A

On the right side.

49
Q

What are metalloids and where are they found?

A

Elements with properties of both metals and non-metals, found between them.

50
Q

What are Noble Gases and their characteristics?

A

Inert gases with full electron shells that don’t react easily.

51
Q

Give examples of Noble Gases.

A
  • Helium
  • Neon
  • Argon
52
Q

What is an element?

A

A pure substance made up of only one type of atom.

53
Q

Define a molecule.

A

A group of two or more atoms bonded together.

54
Q

What is a lattice?

A

A regular, repeating arrangement of atoms, ions, or molecules in a solid.

55
Q

List properties of metals.

A
  • Ductility
  • Malleability
  • Lustre
  • Electrical conductivity
  • Solid state at room temperature (except Mercury)
56
Q

List properties of non-metals.

A
  • Brittleness
  • Low conductivity
  • Can be solid, liquid, or gas at room temperature
57
Q

What is a compound?

A

A substance made from two or more different elements that are chemically bonded together.

58
Q

Differentiate between an element, a molecule, and a compound.

A
  • Element: Pure substance with only one type of atom
  • Molecule: Two or more atoms bonded together
  • Compound: Two or more different elements chemically bonded
59
Q

What is the formula for water?

60
Q

What is the formula for glucose?

A

C₆H₁₂O₆.

61
Q

What is the formula for methane?

62
Q

What is the formula for ammonia?

63
Q

What is the formula for carbon dioxide?

64
Q

What is the formula for carbon monoxide?

65
Q

What are ionic compounds?

A

Compounds that contain metal and non-metal elements.

66
Q

What are covalent compounds?

A

Compounds formed by sharing electrons between non-metal atoms.

67
Q

What is a physical change?

A

A change in form or appearance without altering chemical composition.

68
Q

What is a chemical change?

A

A process that results in the formation of new substances.

69
Q

List signs of a chemical change.

A
  • Colour change
  • Gas production
  • Temperature change
  • New substance formed
  • Odour produced
  • Light or flame produced
70
Q

What is an exothermic reaction?

A

A reaction that releases heat.

71
Q

What is an endothermic reaction?

A

A reaction that absorbs heat.

72
Q

What are reactants in a chemical reaction?

A

The starting substances.

73
Q

What are products in a chemical reaction?

A

The substances produced.

74
Q

What is a word equation in chemistry?

A

A description of a chemical reaction using words.

75
Q

What is a chemical equation?

A

A description of the reaction with symbols and formulas.

76
Q

What does the law of conservation of mass state?

A

The mass of reactants equals the mass of products.

Chemistry Year 8 (1 decks)

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