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Chemistry 2.4 > Chemistry NCEA 2.4 (External; 5 Credits) > Flashcards

Chemistry NCEA 2.4 (External; 5 Credits) Flashcards

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1
Q

Anion

A

When atoms GAIN electrons to form ions

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2
Q

Cation

A

When atoms LOSE electrons to form ions

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3
Q

What does solubility mean?

A

The ability for something to be dissolved in water (liquid)

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4
Q

What are the three types of bonds

A

Ionic, Covalent, Metallic

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5
Q

Do metals have more protons than electrons?

A

Yes - positive charge

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6
Q

Do non-metals have more electrons than protons?

A

Yes - negative charge

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7
Q

What type of solid is a metal?

A

Metallic

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8
Q

What type of solid is a non-metal?

A

Molecular

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9
Q

What type of solid is a metal and a non-metal?

A

Ionic

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10
Q

What types of particles are in a metallic solid?

A

Atoms

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11
Q

What types of particles are in a ionic solid?

A

Ions

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12
Q

What types of particles are in a molecular solid?

A

Molecules

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13
Q

What attractive force is between metal?

A

Metallic bonding

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14
Q

What attractive force is between non-metal and metal?

A

Ionic bonding

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15
Q

What does malleable mean?

A

The ability to change shape without breaking or cracking

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16
Q

What is malleable - metal or non-metal?

A

Metal

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17
Q

What does brittle mean?

A

hard but liable to break easily - fragile

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18
Q

What is brittle - metal or non-metal?

A

Non-metal

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19
Q

Four bonding regions ; The angle

A

109 degrees

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20
Q

Four bonding regions ; The shape

A

4 sticks = Tetrahedral
3 sticks = Trigonal pyramid
2 sticks = bent

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21
Q

Three bonding regions ; The degree

A

120 degrees

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22
Q

Three bonding regions ; The shape

A

3 stick = Triagonal planar

2 stick = bent

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23
Q

Two bonding regions ; The degree

A

180 degrees

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24
Q

Two bonding regions ; The shape

A

Linear

25
Q

Polar bonds are symmetrical? True or False?

A

False

26
Q

Non-polar bonds are symmetrical? True or False?

A

True

27
Q

The formula to find the number of moles of any substances

A

n (mol) = mass / molar mass (gmol-1)

28
Q

What is Endothermic?

A

When a reaction ABSORBS energy

29
Q

What is Exothermic

A

When a reaction RELEASES energy

30
Q

When the delta r H is a positive number it is _____

A

Endothermic

31
Q

When the delta r H is a negative number it is _____

A

Exothermic

32
Q

Reactant above, first is ________

A

Exothermic

33
Q

Product below, first is ________

A

Endothermic

34
Q

Structure of “Polarity”

A

The ______ bond is non-/polar due to difference in electronegativity of the ___ and the ___.

The __( 2, 3 or 4) _____ bonds are/ not spread symmetrically around the _____ shaped molecule therefore the bond dipoles do not/cancel out and overall the molecule is non-/polar.

35
Q

Structure of “shapes of molecules”

A

There are ____(2,3 or 4) regions of negative charge around the central _________ atom, which repel to give maximum separation, into a _______________ arrangement, with a bond angle of ____0.

There are _____(2,3 or 4) bonding regions and _____ (0, 1 or 2) non-bonding regions, therefore the overall shape is _____________.

36
Q

Molecular substances ; Introduction

A

Intro: _________ is a molecular substance made up of non-metal __ and __ atoms covalently bonded together. The molecules are held together by weak intermolecular forces.

37
Q

Molecular substances ; BP/MP

A

BP/MP: These forces do not require much energy to break them, therefore ______ is a (gas at room temperature)/has a low MP/BP.

38
Q

Molecular substances ; Conductivity

A

Conductivity: ______ does not conduct as it does not contain charged particles to carry the electrical charge.

39
Q

Molecular substances ; Maleability

A

Maleability: As the intermolecular forces between the particles are weak, _____ is soft and can be broken up easily.

40
Q

Metallic substances ; Introduction

A

Introduction: (metal)__ consists of (metal)__ atoms held together by non-directional forces between the positive nuclei of the atoms and the delocalised valence electrons.

41
Q

Metallic substances ; MP/BP

A

MP/BP: A lot of energy is required to overcome these strong metallic bonds and therefore ______ has a high MP/BP. (or is a solid at room temperature)

42
Q

Metallic substances ; Malleability/Ductility

A

Malleability/Ductility: Since the attractive forces are non-directional, when pressure is applied, the ___ atoms can move past each other to change shape without the bonds breaking, so ___ is malleable (or ductile).

43
Q

Metallic substances ; Conductivity

A

Conductivity: The valence electrons are free to move throughout the lattice meaning that _____ (metal) can conduct. Solubility: There is no attraction between the ___ atoms and water molecules so ___ is insoluble.

44
Q

Ionic substances ; Introduction

A

Introduction: __________ is an ionic substance made up of positively charged ___+ ions and negatively charged ___- ions. These ions are held together by strong electrostatic forces of attraction in a 3D lattice structure.

45
Q

Ionic substances ; MP/BP

A

MP/BP: A lot of energy is required to overcome these strong ionic bonds and therefore ______ has a high MP/BP. (or is a solid at room temperature)

46
Q

Ionic substances ; Conductivity

A

Conductivity: …and are not able to move, therefore there are no charged particles free to move to conduct the electricity in a solid ionic substance. When molten the ionic bonds are partially overcome and the ions are free to move and carry the charge, therefore the molten ionic substance conducts.

47
Q

Ionic substances ; Maleability

A

Maleability: Ionic substances are not malleable (brittle) as when pressure is applied it forces the ions with the same charge to be next to each other. They will repel each other and the substance will break.

48
Q

Ionic substances ; Solubility

A

Solubility: When added to water, polar water molecules form electrostatic attractions with the ___+ and the ___- ions. The partial negative charge on the oxygen atoms in the water are attracted to the ___+ ions and the partial positive charge on the hydrogen atoms in the water are attracted to the ___- ions, causing the ____ to dissolve. The solute-solvent attractions are strong enough to overcome the solute-solute and solvent - solvent attractions.

49
Q

Covalent networks ; Introduction (4 bonds)

A

Introduction: _______ consists of _____ atoms each covalently bonded to 4 __ atoms in a 3D lattice structure. These covalent bonds are strong.

50
Q

Covalent networks ; MP/BP (4 bonds)

A

MP/BP: The strong covalent bonds require a lot of energy to break, so the melting point of ______ is very high.

51
Q

Covalent networks ; Hardness (4 bonds)

A

Hardness: The strong covalent bonds make it very difficult to break ______.

52
Q

Covalent networks ; Conductivity (4 bonds)

A

Conductivity: All of the valence electrons are involved in bonding so there are no free electrons to carry the charge, so ______ does not conduct.

53
Q

Covalent networks ; Introduction (3 bonds)

A

Introduction: __________consists of C atoms each covalently bonded to _________other _______ atoms in layered arrangement with ________ intermolecular forces of attraction between the layers or sheets. (Note: no layers in graphene or nanotubes etc.)

54
Q

Covalent networks ; MP (3 bonds)

A

MP: It would require a lot of energy to break the strong ________ bonds, therefore _________ has a high melting point.

55
Q

Covalent networks ; Hardness (3 bonds)

A

Hardness: Although the bonds between the covalently bonded carbon atoms in the layers are strong, the forces between the layers are weak, resulting in the layers sliding over each other. Therefore _________ is a soft substance.

56
Q

Covalent networks ; Conductivity (3 bonds)

A

Conductivity: As each carbon atom is bonded to three others in the layers, each has one valence electron, which is free to move. These delocalised electrons result in ________ conducting electricity.

57
Q

What is conductivity?

A

Conductivity is the measure of the ease at which an electric charge or heat can pass through a material.

58
Q

What force does a molecular solid have?

A

Intermolecular force

Chemistry 2.4 (1 decks)

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