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3U CHEMISTRY > 1.5 CHEMICAL COMPOUNDS & PROPERTIES > Flashcards

1.5 CHEMICAL COMPOUNDS & PROPERTIES Flashcards

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1
Q

What is the charge of carbon?

A

+/-4

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2
Q

given:

solid

44ºC melting point

280ºC boiling point

not soluble

A

non-polar covalent, not soluble

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3
Q

What is another name for hydrogen carbonate?

A

bicarbonate

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4
Q

______ temp will _______ speed of particle.

A

increasing temp will increase speed of particle.

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5
Q

What is the formula for:

di-iodine pentasulphide

A

I2S5

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6
Q

What is the name for:

Mn(HCO3)4

A

manganese (IV) bicarbonate

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7
Q

Solids have what kind of bonds?

A

very strong bonds between particles will form solids

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8
Q

What is the name for FeN?

A

iron (III) nitride

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9
Q

given:

solid at room temp.

730ºC melting point

1380ºC boiling point

soluble in water

A

ionic, because of the high melting/boiling point AND soluble in water.

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10
Q

What two polyatomic exceptions are positively charged? What is their suffix?

A

hydroxide and ammonium, ending in -ate.

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11
Q

All substances are made up of _______ and they are in ___________ motion. The motions are _______, ________, ________.

A

All substances are made up of particles and they are in constant motion. The motions are linear, rotational, vibrational.

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12
Q

What state of matter has the weakest forces?

A

Gases.

When contained will expand to fill vessel, but if uncontained will usually drift apart.

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13
Q

Chemical formula for:

tin (IV) sulphate

A

Sn(SO4)2

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14
Q

Special type of dipole-dipole force.

A

Hydrogen bonds.

between hydrogen and fluorine, oxygen and nitrogen ONLY because they are extremely electronegative. v.strong bond

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15
Q

What is it called when covalent bonds share electrons equally?

A

Pure/non-polar covalent bond

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16
Q

What is the formula for bicarbonate?

A

HCO3-

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17
Q

Chemical formula for:

mercury (I) phosphide

A

Hg3P

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18
Q

A type of ion that has more electrons than protons

A

anions.

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19
Q

What are the properties of polar covalent molecules?

A
  • can be solid, liquid or gas at room temp, depending on molecule size
  • generally v low melting/boiling point
  • soluble if not too large
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20
Q

What is the name for Hg2C?

A

mercury (III) carbide

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21
Q

What naming system do we use to show the different of charge of multivalent metals/elements?

A

Stock Naming, using roman numerals.

The roman number follows the name of the element and shows the positive charge.

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22
Q

What is the chemical name for Li2O?

A

Lithium oxide

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23
Q

Intermolecular forces can change the ___________ at room temp.

A

state of matter

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24
Q

Are most polyatomic ions positively or negatively charged?

A

negatively

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25
Q

Name for:

SnS2

A

tin (II) sulphide

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26
Q

A cation is?

A

a positive ion. more protons than electrons

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27
Q

What are the propteries of non-polar covalent molecules?

A
  • can be any state at room temp, depending on molecule size
  • gen v low melting/boiling point, lower than polar molecule of same size
  • not soluble
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28
Q

What is name for Cu(NO3)2?

A

copper (II) nitrate

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29
Q

Formula for:

ammonium phosphate

A

(NH4)3PO4

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30
Q

What is an emulsifier?

A

An emulsifier keeps polar and non-polar ingredients bonded though they naturally wouldn’t be. It has a positive and negative end to keep ingredients bonded. Can be natural or chemical.

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31
Q

Melting point

A

is temp needed for a solid to become a liquid

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32
Q

What is the name for:

Cl2O

A

dichlorine oxide

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33
Q

Ionic compounds are composed of ______ ions.

A

alternating. (positive and negative)

34
Q

What is the chemical name for:

KBr

A

potassium bromide

35
Q

What type of substances are always solid at room temp?

A

Ionic substances.

36
Q

What is the chemical formula for calcium chloride?

A

CaCl2

37
Q

Makes water liquid at room temp

A

hydrogen bonds

38
Q

Kinetic Molecular Theory can be thought of as “__________ theory”

A

moving particle theory

39
Q

What state is water?

A

liquid

40
Q

Are bonds between ions stronger or are bonds between molecules stronger?

A

bonds betwen ions are stonger because ions have charges and molecules do not.

41
Q

The ______ the distance between particles the _____ the attraction.

A

The further the distance between particles the lesser the attraction.

42
Q

Which state of matter allows particles to stay close together but still move freely to flow and change shape?

A

liquids. these forces are stronger than gases.

43
Q

When learning how to names and formulas, it is important to differentiate between ________ and _________?

A

vocabulary vs grammar.

vocabulary is words, grammar is how to use.

oxygen vs zinc oxide.

44
Q

If a molecule is charged, it is called a _______________

A

polyatomic ion

45
Q

Forces that cause attraction between molecules is called ____________________.

A

Forces that cause attraction between molecules is called intermolecular forces.

46
Q

Between salt and vinegar, which has stronger attractive forces?

A

salt. because it is a solid at room temp and vinegar is a liquid at room temp.

47
Q

The small separation of charge in a bond is called a ______.

A

The small separation of charge in a bond is called a dipole.

48
Q

A non-metal and non-metal makes up a _______ compound

A

covalent

49
Q

What is solubility?

A

refers to substance’s ability to dissolve with water

50
Q

What temp is considered room temp?

A

25ºC

51
Q

Are ionic substances soluble in water?

A

Yes, many are.

52
Q

A polyatomic ion is a _______ molecule.

A

charged

53
Q

Freezing point

A

is the same as melting point

54
Q

What is the chemical formula for:

copper (II) phosphide

A

Cu3P2

55
Q

Define miscibility

A

is a substances ability to mix.

56
Q

Name for:

NF5

A

nitrogen pentafluoride

57
Q

Boiling point

A

temp needed for a liquid to become gaseous

58
Q

atoms that bond together covalently form ____________

A

molecules

59
Q

What are molecules called when they only have pure covalent bonds?

A

non-polar molecules

60
Q

What are London Forces?

A

a temporary bond between molecules. one end of the bond becomes positive and one end becomes negative therefore becoming attracted to each other. v weak bond.

61
Q

what is the chemical name for:

PbSO4

A

lead (II) sulfate

62
Q

given:

gas

  • 115ºC melting point
  • 85ºC boiling point

soluble

A

polar covalent. low melting/boiling, water soluble.

63
Q

What electrons in a polar covalent bond are always closer to which atom?

A

The higher electronegative one

64
Q

Describe the functions and properties of soap that allows it to clean things.

A

Soap has polar and non-polar ends and is relatively large. It forms miscelles when combined with water. The non-polar tails dissolve droplets of oil forming a capsule around the oil. Polar head protrudes with water. keeps it together so it can be washed away.

65
Q

Name for:

(NH4)2CO3

A

ammonium carbonate

66
Q

Group 1 elements gain a charge of what?

A

1+

67
Q

A non metal and metal makes a what?

A

binary ionic compound

68
Q

negatively charged polyatomic ions ALL contain ______, called ____ - ions.

A

oxygen. oxy-ions

69
Q

Define immiscible

A

liquids that do not dissolve.

70
Q

What is the chemical formula for cadmium bromide?

A

CdBr2

71
Q

What is the name for:

CBr4

A

carbon tetrabromide

72
Q

What factors determine strength of London Forces?

A
  • increase in contact area (more molecules)
  • polarizability, increase in molecular size
73
Q

What does the different charge do?

A

It changes the property of the element. Like iron. Iron (II) powder is black. iron (III) powder is red.

74
Q

given:

gas at room temp

  • 101ºC melting point
  • 34ºC boiling point

not soluble

A

non-polar covalent because of low melting and boiling and NOT soluble

75
Q

particles attract each other.

A

Rule of KMT and the particle theory.

76
Q

What are Dipole Forces?

A

dipole forces are in polar molecules, partial charges. Stronger than london forces. Slightly higher charge one one side, slightly lower on the other.

77
Q

What is the name for elements that have more than one possible charge?

A

multivalent metals

example: iron has charge of 2+ or 3+

78
Q

What is the charge on binary ionic compounds?

A

zero.

79
Q

What is the chemical formula for:

bismuth (V) phosphide

A

Bi3P5

80
Q

When naming binary ionic compounds, which atom gets the -ide ending?

A

The altered non-metal gets the -ide ending.

For example: Lithium + chlorine = lithium chloride

81
Q

What is the relative melting and boiling point for ionic substances?

A

generally very high

3U CHEMISTRY (2 decks)

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