Chemistry: Chapter 3 (Atoms Combining) Flashcards

1
Q

Definition of Element

A

A substance that contains only one kind of atom and cannot be broken down further into another substance.

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2
Q

Definition of Compounds

A

A substance that is made of atoms of different elements that are chemically bonded together.

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3
Q

Definition of Mixture

A

Different substances that are physically mixed together.

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4
Q

What are the 3 signs of chemical change?

A
  • one or more new chemical substances are formed
  • energy is taken in or given out during the reaction
  • the change is usually difficult to reverse
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5
Q

What are 2 ways to reverse a chemical change?

A

Heating with carbon and electrolysis

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6
Q

How to differenciate physical changes from chemical changes?

A

If it produces a new substance, it is chemical change. If it does not, it is physical change.

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7
Q

3 signs of chemical reactions

A
  • colour change
  • sweet smell / foul stench
  • temperature change
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8
Q

Why do atoms form bonds?

A

Atms form bonds together in order to obtain a full valence electron shell.

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9
Q

Which group of gases are unreactive?

A

Group VIII, the noble gases

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10
Q

Why does sodium gain a single positive charge?

A

When the sodium atom donates an electron, the number of protons is one more than electrons.

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11
Q

What are positive and negative ions called?

A

Cation (+) and Anion (-)

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12
Q

Why do atoms of Group VIII not form ions?

A

They have a full electron shell and do not need to receive or donate electrons, they are unreactive.

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13
Q

Definition of Ionic Bond

A

A strong electrostatic attraction between ions of opposite charge.

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14
Q

Definition of Lattice

A

3D structure of regular and repeating pattern of oppositely charged ions.

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15
Q

What is the overall charge of the compound NaCl?

A

No overall charge, the charges on the ions cancel each other out.

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16
Q

Which element goes at the front of a compound name?

A

The element with a positive charge

17
Q

Definition of Molecules

A

Two or more atoms held together by covalent bonds.

18
Q

Why do carbon atoms not form ions?

A

Carbon and other elements in Group IV would have to lose or gain many electrons, which would take too much energy, thus carbon only shares electrons.

19
Q

Why do non-metal elements not form ionic bonds with each other?

A

Non-metals only receive electrons to form anions, anions will repel each other so it cannot form ionic bonding.

20
Q

Definition of Covalent Bond

A

Atoms gaining full electron shells by sharing electrons with each other.

21
Q

Definition of Regular Lattice

A

Regular lattice grows in all directions, giving a crystal-like structure.

22
Q

What is the weak force in between molecultes called?

A

Intermolecular force

23
Q

Properties of Ionic Compounds

A
  • high MP and BP
  • usually soluble in water
  • can conduct electricity when dissolved or molten (ions are not free to move in solid state)
24
Q

Properties of Covalent Compounds

A
  • low MP and BP
  • usually insoluble in water
  • cannot conduct electricity (no charge bc no ions)
25
Q

What are the two types of covalent structures?

A

Simple molecular structure and giant covalent structure

26
Q

What are the three giant covalent structures?

A

Graphite, diamond and silica

27
Q

Properties of Diamond and Silica

A
  • very hard (held in place by 4 strong covalent bonds)
  • high melting point
  • cannot conduct electricity (no moving electrons)
28
Q

Properties of Graphite

A
  • soft and slippery (layers can slide over each other)
  • good conductor of electricity (delocalised electrons moving between layers)
29
Q

Uses of Graphite

A
  • lubricant in engines
  • electrodes in electrolysis
30
Q

Use of Diamond

A
  • tools for drilling and cutting
31
Q

Uses of Silica

A
  • in bricks for lining furnaces
  • sandpaper
32
Q

Definition of Allotropes

A

Different forms of an element

33
Q

Definition of Metallic Bond

A

The electrostatic attraction between the positive ions in a ‘sea’ of delocalised electron that move freely.

34
Q

What force are metal ions held together by?

A

Electrostatic attraction

35
Q

Properties of Metals

A
  • high melting point (high heat to overcome strong electrostatic forces between metal ions and delocalised electrons)
  • malleable and ductile (layers of metal ions can slide over each other)
  • good conductors of heat (free electrons take in heat energy, which makes them move faster)
  • good conductors of electricity( free electrons move through the lattice as a current of electricity, when a voltage is applied across the metal.
36
Q

Which metal is the best conductor?

A

Silver (copper is next but is used more often as it is cheaper)

37
Q

Which bonds use electrostatic attraction?

A

Ionic bonding and Metallic bonding

ionic: cation & anion
metallic: positive metal ions & sea of delocalised electrons

38
Q

What does it mean to be malleable and ductile?

A

Malleable: can be bent and pressed into shape
Ductile: can be drawn into wires