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CheMisTrY - Elements Of Life > EL.7 > Flashcards

EL.7 Flashcards

Bonding, structure, properties, and precipitates

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1
Q

What is the formula of sulfuric acid?

A

H2SO4

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2
Q

What is the formula for hydrochloric acid?

A

HCl

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3
Q

What is the formula for nitric acid?

A

HNO3

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4
Q

What ion does acids produce?

A

H+

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5
Q

How do group 1 and 2 metals become ions?

A

They lose their outer shell electrons to become positively charged ions.

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6
Q

How do non metals become ions?

A

The gain electrons to become negative charged ions..

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7
Q

What are positively charged ions also known as?

A

Cations.

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8
Q

What are negatively charged ions also known as?

A

Anions.

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9
Q

Why are -3 ions so rare?

A

Because once an anion is already -1, it become harder to attract another electron as both particles have the same charge and repel each other, making -2 very difficult to achieve and -3 even more rare.

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10
Q

What happens in ionic bonding?

A

Electrons are transferred from the metal atoms to the non metal atoms, forming ions with a closed shell stable structure like that of noble gas. The cation and anion are held together by a strong attraction between their opposite charges.

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11
Q

What is the strong attraction between the cation and anions’ opposite charges also known as?

A

Electrostatic force/bond.

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12
Q

How is a solid ionic compound held together?

A

Each ion forms electrostatic bond with many other ions of opposite charge and the ions build up into a giant lattice.

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13
Q

Which part of an anion’s name indicates it’s a negatively charged ion?

A

xxx-ide, eg. fluoride, oxide, hydroxide.

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14
Q

What bond holds together groups of atoms in a complex ion?

A

Covalent bond.

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15
Q

What does the overall charge of an ionic compound have to be?

A

0

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16
Q

There are four main ways of making salt from acids and bases, what are the products produced from each of these reactions?

  1. acid + alkali → _ + _
  2. acid +base → _ + _
  3. acid + carbonate → _ + _ + _
  4. acid + metal → _ + _
A
  1. acid + alkali → salt + water
  2. acid +base → salt + water
  3. acid + carbonate → salt + water + carbon dioxide
  4. acid + metal → salt + hydrogen
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17
Q

What are some ionic compounds that are not soluble?

A
  • barium, calcium, lead and silver sulfates.
  • silver and lead halides (chlorides, bromides, iodides).
  • all metal carbonates.
  • metal hydroxides (except Group 1 hydroxides and ammonium hydroxide).
18
Q

Why are aqueous solutions of salt able to conduct electricity?

A

When ionic compounds dissolve in water, ions are separated and surrounded by water molecules and behave independently of each other. They are able to move around freely and carry charges.

19
Q

When ions are in solution, do both types of ions get involved in a reaction of ionic substance?

A

No, it often involves only one of the two types of ion.

20
Q

What are the ions not involved in the reaction known as?

A

Spectator ions.

21
Q

What is an ionic equation?

A

The equation that only shows the ions that take place in the reaction, it leaves out the spectator ions which do not do anything.

22
Q

What are the state symbols for the following physical states of chemicals:

  1. solid
  2. liquid
  3. gas
  4. aqueous solution
A
  1. [s]
  2. [l]
  3. [g]
  4. [aq]
23
Q

What is the precipitation test for Cu2+ copper ions?

A

Add sodium hydroxide and a blue precipitate of copper hydroxide will form.
Cu2+[aq] + 2OH-[aq] → Cu(OH)2[s]

24
Q

What is the precipitation test for Fe2+ iron(II) ions?

A

Add sodium hydroxide and a green precipitate of iron(II) hydroxide will form.
Fe2+[aq] + 2OH-[aq] → Fe(OH)2[s]

25
Q

What is the precipitation test for Fe3+ iron(III) ions?

A

Add sodium hydroxide and a brown precipitate of iron(II) hydroxide will form.
Fe3+[aq] + 3OH-[aq] → Fe(OH)3[s]

26
Q

What is the precipitation test for Pb2+ lead ions?

A

Add potassium iodide and a yellow precipitate of lead iodide will form.
Pb2+[aq] + 2I-[aq] → PbI2[s]

27
Q

What is the precipitation test for Cl- chloride ions?

A

Add silver nitrate and a white precipitate of silver chloride will form.
Ag+[aq] + Cl-[aq] → AgCl[s]

28
Q

What is the precipitation test for Br- bromide ions?

A

Add silver nitrate and a cream precipitate of silver bromide will form.
Ag+[aq] + Br-[aq] → AgBr[s]

29
Q

What is the precipitation test for I- iodide ions?

A

Add silver nitrate and a pale yellow precipitate of silver iodide will form.
Ag+[aq] + I-[aq] → AgI[s]

30
Q

What is the precipitation test for SO42- sulfate ions?

A

Add barium chloride and a white precipitate of barium sulfate will form.
Ba2+[aq] + SO42-[aq] → BaSO4[s]

31
Q

What physical state are ionic compounds normally in at room temperature and pressure?

A

Solids.

32
Q

What is the structure of solid ionic compounds called and what is it?

A

Lattice structure, it’s when positive and negative ions are arranged in a repeating manner in all three dimensions. It is also why ionic compounds often form regularly shaped crystals.

33
Q

What type of ion take on the suffix -ate?

A

Oxyanion, XOyz-, eg. sulfate SO42-. Contains oxygen and another element and is negative.

34
Q

What is the relative comparison between the size of an anion and its corresponding atom?

A

Anions are always bigger than its corresponding atom.

35
Q

What is the relative comparison between the size of a cation and its corresponding atom?

A

Cations are always smaller than its corresponding atom.

36
Q

What force holds metallic structures together?

A

The electrostatic attraction between the metal cations and delocalized electrons.

37
Q

How many carbons does each carbon atom bond to in diamond’s giant covalent network?

A

Each carbon is bonded to another 4 carbon atoms in a tetrahedral shape.

38
Q

What are some properties of ionic compounds regarding:

a) melting/boiling points
b) hardness
c) electrical conductivity
d) solubility in water

A

a) high
b) hard but brittle
c) conduct when molten or dissolve in water.
d) often soluble

39
Q

What are some properties of giant covalent networks regarding:

a) melting/boiling points
b) hardness
c) electrical conductivity
d) solubility in water

A

a) very high
b) very hard, if three dimensional
c) do not conduct, except graphite
d) insoluble

40
Q

What are some properties of metallic compounds regarding:

a) melting/boiling points
b) hardness
c) electrical conductivity
d) solubility in water

A

a) generally high
b) hard but malleable
c) conduct when solid or liquid
d) insoluble but react with water

41
Q

What are some properties of simple covalent molecules regarding:

a) melting/boiling points
b) hardness
c) electrical conductivity
d) solubility in water

A

a) low, typically gases or liquids at room temperature
b) soft
c) do not conduct
d) usually insoluble, although some contain groups that are able to form hydrogen bond with water

42
Q

What are some properties of macromolecule e.g. polymers regarding:

a) melting/boiling points
b) hardness
c) electrical conductivity
d) solubility in water

A

a) moderate, often decompose on heating
b) variable, often quite flexible
c) do not normally conduct
d) usually insoluble

CheMisTrY - Elements Of Life (9 decks)

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