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Science > Bk2 Ch2 Atoms > Flashcards

Bk2 Ch2 Atoms Flashcards

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1
Q

Element (definition)

A

<p>An element is a pure substance composed of only one type of atom.</p>

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1
Q

<p>possible ways to break down a substance</p>

A

<p>burning or using acids or other chemicals.</p>

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2
Q

<p>There are how many naturally occurring elements</p>

A

<p>92</p>

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2
Q

<p>There are how many synthetic elements</p>

A

<p>over 20</p>

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3
Q

<p>Name two metals and give examples of their uses</p>

A

<p>aluminium is used to form cooking utensils, copper for electrical wires and plumbing pipes.</p>

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3
Q

<p>Name two non-metals and give examples of their uses</p>

A

<p>Nitrogen is used for making fertilisers, carbon (diamond) for jewellery and cutting tools.</p>

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4
Q

<p>Describe the connection between atoms and elements.</p>

A

<p>Atoms which are the same make up elements.</p>

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4
Q

<p>Most abundant elements on earth</p>

A

<p>oxygen 47%, silicon 28%, aluminium 8%, iron 5%</p>

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5
Q

<p>The Hindenburg airship (or Zeppelin) was filled with the element</p>

A

<p>hydrogen</p>

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5
Q

<p>Of the 106 known elements, how many metals and non-metals?</p>

A

<p>84 metals, 22 non-metals</p>

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6
Q

<p>All metallic elements are solids at room temperature except for</p>

A

<p>mercury</p>

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6
Q

<p>atom (definition)</p>

A

<p>the smallest piece of a substance that is still that substance.</p>

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7
Q

<p>The word ‘atom’ comes from the Greek word</p>

A

<p>atomos, meaning ‘that which cannot be divided’.</p>

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7
Q

<p>What is the lightest atom?</p>

A

<p>Hydrogen</p>

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8
Q

<p>Name two heavy atoms</p>

A

<p>Hassium, Meitnerium</p>

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8
Q

<p>Atoms are made up of…</p>

A

<p>Protons, neutrons & electrons</p>

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9
Q

<p>Name the three naturally occurring isotopes of Hydrogen.</p>

A

<p>1. protium 2. deuterium 3. tritium</p>

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9
Q

<p>Atoms are most stable when…</p>

A

<p>their outer shells are filled.</p>

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10
Q

<p>1 mole = </p>

A

<p>6.022 x 10^23 (ten to power of 23) </p>

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10
Q

<p>1 mole of an element is..</p>

A

<p>it's atomic weight in grams</p>

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11
Q

<p>ion (definition)</p>

A

<p>a charged atom</p>

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11
Q

<p>Metals are</p>

A

<p>electron donors</p>

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12
Q

<p>Non-Metals are</p>

A

<p>electron acceptors</p>

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12
Q

<p>Compound (definition)</p>

A

<p>A substance formed by two or more elements combined in a fixed ratio.</p>

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13
Q

<p>Using examples, identify the two types of compound structures.</p>

A

<p>Molecule (eg: water H2O, Oxygen O2) and Lattice (eg: Sodium Chloride NaCl, Quartz SiO2)</p>

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13
Q

<p>Molecule (definition)</p>

A

<p>Two or more atoms chemically combined.</p>

14
Q

<p>Lattice (definition)</p>

A

<p>A regular array of atoms chemically combined.</p>

14
Q

<p>Mixture (definition)</p>

A

<p>A mixture is a collection of different substances (elements or compounds). These substances are not bonded together and no new substance is formed when they are combined.</p>

15
Q

<p>A physical change occurs when…</p>

A

<p>a substance changes, but no new substance is formed.</p>

15
Q

<p>Physical changes occur when the state of a substance changes. Eg:</p>

A

<p>melting, evaporation, freezing, condensing (or a substance is crushed, ground or cut into smaller pieces.)</p>

15
Q

<p>A chemical change or chemical reaction occurs whenever…</p>

A

<p>a new substance forms.</p>

15
Q

<p>Indications of a chemical change…</p>

A

<p>Production of bubbles of gas. A change in colour. The production of heat (exothermic) or light. A drop in temperature (endothermic). A solid is formed (precipitate).</p>

15
Q

<p>The substances present before the chemical reaction has occurred are called the…</p>

A

<p>reactants.</p>

15
Q

<p>The chemicals formed by the reaction are called the…</p>

A

<p>products.</p>

15
Q

<p>Combination reactions (definition)</p>

A

<p>where two or more reactants join together to form one new substance.</p>

15
Q

<p>Combination reactions (example)</p>

A

<p>rusting of a metal: iron + oxygen -> iron oxide</p>

15
Q

Combination reactions are also called…

A

synthesis reactions.

15
Q

Decomposition reactions (definition)

A

A single reactant breaking down or decomposing into two or more new substances.

15
Q

Decomposition reactions (example)

A

Water can be broken down using electricity to produce oxygen gas and hydrogen gas.

15
Q

Precipitation reactions (definition)

A

when a solid forms when two solutions are mixed together.

15
Q

Combustion reactions (definition)

A

Combustion reactions happen whenever something burns or explodes.

15
Q

Combustion reactions (example)

A

Carbon may be burnt to produce carbon dioxide gas. carbon + oxygen -> carbon dioxide

15
Q

Reaction rate can be affected by:

A

The amount or concentration of reactants. Temperature. Surface area. Catalysts (helper chemicals)

15
Q

Catalyst (definition)

A

A substance that increases the rate of a chemical reaction without itself undergoing any permanent chemical change.

15
Q

What are enzymes?

A

Special types of catalysts called enzymes are found in our bodies. Digestive enzymes help break down large molecules such as starch into smaller molecules such as glucose.

15
Q

Explain what is meant by each of the following when written in chemical equations: (s), (l), (g), (aq), ->

A

solid, liquid, gas, aqueous,

15
Q

the atomic number is

A

the number of protons in the nucleus.

15
Q

the mass number is

A

the number of protons and neutrons in the nucleus.

15
Q

To find the number of neutrons, you subtract…

A

the atomic number from the mass number.

15
Q

Number of electrons =

A

number of protons = atomic number

15
Q

The original idea of a small particle called the atom came from..

A

the ancient Greeks, some 2000 years ago.

16
Q

In 1808 which English chemist supports the idea of atoms as solid balls?

A

John Dalton

17
Q

In 1897 who discovers electrons?

A

Sir Joseph John Thomson (Great Britain)

18
Q

In 1903, who proposes the ‘plum pudding’ model of a positively charged ‘dough’ with negatively charged electrons embedded in it?

A

Sir Joseph John Thomson (Great Britain)

19
Q

In 1911, who proposes a nuclear model in which negatively charged electrons orbit a positive nucleus, with most of the atom being empty space?

A

Ernest Rutherford, a New Zealand born physicist and student of Thomson.

20
Q

In 1913, who extends Rutherford’s model to include electron shells?

A

Niels Bohr, a Danish physicist and assistant to Rutherford.

21
Q

In 1914, who discovers the proton?

A

Ernest Rutherford

22
Q

In 1932, who discovers neutrons?

A

James Chadwick (Great Britain)

23
Q

Atoms are mainly what?

A

empty space.

24
Q

The model of the atom used today is the…

A

Rutherford–Bohr model.

25
Q

Protons and neutrons have about the same mass, while electrons have…

A

about 1/2000th the mass of protons and neutrons.

26
Q

In what year were electrons discovered?

A

1897

27
Q

In what year were protons discovered?

A

1914

28
Q

In what year were neutrons discovered?

A

1932

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