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Chem 101 > Specific Fun things about Specific Elements, Groups, and Compounds > Flashcards

Specific Fun things about Specific Elements, Groups, and Compounds Flashcards

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1
Q

What’s the main thing that makes hydrogen so special?

A

It’s very small

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2
Q

Industial Methods of Creating Hydrogen

A

Water-gas shift reaction
C (solid) + H2O (gas) → CO (solid) + H2 (gas)

Steam Hydrocarbon Reforming
CH4 (solid) + H2O (gas) → CO2 (gas) + 3H2 (gas)
Note the CH4 can be any hydrocarbon

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3
Q

What do you get when a Hydrogeen reacts with metal?

A

Ionic Hydrides

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4
Q

What happens when a hydrogen reacts with a nonmetal?

A

You get a covalent compound

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5
Q

What happens when hydrogen mets transistion elements

A

Metal hydrides (Different from ionic hydrides)

The H2 molecules and H atoms occupy the holes (empty spaces) of the crystal structure of the transition elements
- Good for storage
- No single stoichimetic formula due to the variable amounts of hydrogen that can get in

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6
Q

How do we use hydrogen?

A

Haber Process
N2 (gas) + 3H2 (gas) → 2NH3 (gas)

Hydrogenation of Vegitible Oils

Alternative Fuel
H2 (gas) + 1/2O2 ( gas) → H2O (gas) + heat
- This is clean fuel

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7
Q

What makes hydrogen so hard to use as fuel effectivly?

A
  • H2 (gas) is very flamible and burns explosivly with O2
  • The production of H2 is not clean
  • Special containers are required to store the H2 under high pressure
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8
Q

Atomic and Physical Properties of Group 1

A

Alkali Metals
- Largest atomic size
- Lower densities
- Soft
- Malleable and ductile (able to be made into wire?)
- Good conductors
- Low melting and boiling points

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9
Q

Reactivity of Group 1

A

Very reactive
- wants to lose electrons
- Reacts spontaniously with O2 and H2O
- Reactions with O2 may create oxides, peroxides, and superoxides

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10
Q

Common uses for Gp 1 Elements?

A

Na is used in street lights
KCl is used in fertilizer

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11
Q

What makes this element weird?

Lithium

A

Group 1 Element
- Smallest Alkeli Metal
Forms Li2O with O2
- Li^+ and O^2-
- Interacts better with the smaller O^2- molecule than the larger O^- Molecule

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12
Q

What makes this element weird?

Berillium

A

Group 2
- Smaller and has a higher electronegativity
- Strong Covalent Character
- BeO is an amphoteric oxide
- Tends to form polymeric structures in the solid state

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13
Q

What makes this element weird?

Boron

A

Group 13
- High melting point, black, hard
- Hydrates are called Boranes
- Very Reactive, wants to complete the octet
- Dimerizes Easily

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14
Q

Describe

Aluminum

A

Group 13
- Most abundant element in the Earth’s crust
- High thermal and electical conductivity
- Forms covalent compounds with non-metals
- Dimerizes

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15
Q

Describe

Gallium

A

Group 13
- Low melting point: 29.8 C
- High boiling point: 2100 C
- Used as a replacement for mercury in thermometers due to the high range between melting and boiling points

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16
Q

Differences between:

Carbon and Silicon

A

Group 14
1. C-C single bonds are common, while Si-Si single bonds are not
2. C makes multiple bonds with other C atoms, Si-Si multilple bonds do not exist
3. Oxides of C and Si
- C oxides form molecular compounds, and may form multiple bonds
- Si oxides form giant covalent structures, and only have single bonds

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17
Q

Whats the fancy name for Group 15?

A

pnicogens

18
Q

Whats the fancy name for group 16?

A

chalcogens

19
Q

What are the two types are phosphorus that we studied?

A

White and Red

20
Q

What are the differences between white and red phosphorus?

A

White
- Waxy, solid
- Toxic
- Low melting point
- Strained

Red
- Solid
- Non-toxic
- High melting point
- Not strained
- Used to make meth

21
Q

Industrial Applications of Boron

A
  • Boric acid (white solid) is used to dilute aqueous solutions, dispersed in pawder as as disinfectant, used to make fiberglass
  • Boron-containing glasses are reslistant to thermal shock
22
Q

Where do you find boron and how do you exctract it?

A

Found in borate minerals, Exctracted by converting then reducing

23
Q

Oxyacides of Nitrogen

A

Nitrous Acid HNO2
O.S. of N = +3
- Used in organic synthesis

Nitric Acid HNO3
O.S. of N = +5
- made via the Oswald process
- used to make fertalizers and explosive

24
Q

Oxyacides of Phosphorus

A

Phosphorous acid: H3PO3
O.S. of P = +3
- diprotic acid (one of the H’s is not ionizable)

Phosphoric Acid: H3PO4
O.S. of P = +5
- Triprotic acid

25
Q

Common Oxides of Nitrogen

A

N2O
- Colourless, sweet-smelling gas
- Used as dental anasthetic, in recreational drugs, and as aerosol propellant in whipped cream

NO
- Colourless gas
- Part of the nitrogen fixation cycle

26
Q

Oxides of Phosphorus

A

P4O6
- White, waxy solid
- Formed in reactions with limited O2

P4O10
- White solid
- Formed in reactions with excess O2

27
Q

Where do you typically find oxygen?

A

O2
- Paramagnetic
- Exctracted from the atmophere via fractional distillation

O3
- Pungange dimagnetic gas
- low boiling point
- Toxic to people, but protects the earth from UV rays, so theres that

28
Q

Describe

Sulfur

A

Group 16
- Tends to from bonds with itself
- yellow sulfur, S8, is the most stable version of it
- Important in making fertilizers and other chemicals
- Strong O.A.
- Good dehydrating agent

29
Q

Describe

Flurine

A

Group 17
- The most elecronegative element
- O.N. is allways -1 in compounds
- Never double bonds

30
Q

Atomic and Physical properites of Group 2

A

Alkeline Earth Metals
- Harder and higher melting points than Alkali Metals (higher lattice energy = higher ionic charge = higher melting point)
- Less reactive than Alkali metals, but still very reactive
- Naturaly found in ionic compounds
- Reducing agents
- Reacts with water
M (solid) + 2H2O (liquid) → M(OH)2 (aq) + H2 (gas)
- Often found as carbonates
- Obtained by reduction via eletrolysis of their molten salts
M^2+ (liquid) + 2e → M

31
Q

Atomic and Physical Properties of Group 18

A

Nobel Gases
- Unreactive
- Low melting and boiling points
- May create compounds under lab conditions

32
Q

What are the types of oxides?

A

Acidic Oxides - Oxides of non-metals
- Molecular compounds
- Produce hydronium ions with water
- React with bases

Basic Oxides - Ocides of metals
- Oxides of group 1 and 2 (exept BeO0
- Produce hydroxide ions with water
- React with acids

Amphoteric Oxides - properties of both acid and base
- Does not allways react with water
- Includes BeO
- Only react with acids and bases

33
Q

Acidic Oxides

A

Oxides of non-metals
- Molecular compounds
- Produce hydronium ions with water
- React with bases

34
Q

Basic Oxides

A

Ocides of metals
- Oxides of group 1 and 2 (exept BeO0
- Produce hydroxide ions with water
- React with acids

35
Q

Amphoteric Oxides

A

Amphoteric Oxides - properties of both acid and base
- Does not allways react with water
- Includes BeO
- Only react with acids and bases

36
Q

What makes a good oxidition agent?

A

Molecules are compounds with elements in high (+) oxidation states

37
Q

What makes a good reducing agent?

A

Molecules are compounds with elements in low (-) oxidation states

38
Q

Does Oxidative power of halogens increase or decrease down the group

A

Oxidative power decreases down the group

39
Q

In Group 1 and Group 2, does reducing power increase or decrease down the group

A

It increases down the group
- The lower the I.E., the more reducing it is
- Larger atoms have lower I.E. and are more reducing

40
Q

What is the oxidation state trends of Gp. 15?

A

In ionic compounds, N and P tend to have O.S of 3-

In covalent compounds, the O.S ranges from -3 to +5
- As you procced down the group negative oxidation states become less stable until +3 is the only common O.S. for Bi

41
Q

Uses for Nitrogen?

A
  • Fertilizer (Made via the Haber Process)
  • inert blanketing gas for packaging
  • Useful cyrogen
42
Q

What types of oxydes can alkali metals make?

In exess of oxygen

A

Li2O → 2Li^+ + O^2-
This is with an oxide

Na2O2 → 2Na^+ + O2^2-
This is a peroxide

MO2 → M + O2^(1/2)-
This is a superoxide

The oxygen molecules get bigger as you go down the row

Chem 101 (4 decks)

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