Specific Fun things about Specific Elements, Groups, and Compounds Flashcards
What’s the main thing that makes hydrogen so special?
It’s very small
Industial Methods of Creating Hydrogen
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
What do you get when a Hydrogeen reacts with metal?
Ionic Hydrides
What happens when a hydrogen reacts with a nonmetal?
You get a covalent compound
What happens when hydrogen mets transistion elements
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
How do we use hydrogen?
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
What makes hydrogen so hard to use as fuel effectivly?
- 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
Atomic and Physical Properties of Group 1
Alkali Metals
- Largest atomic size
- Lower densities
- Soft
- Malleable and ductile (able to be made into wire?)
- Good conductors
- Low melting and boiling points
Reactivity of Group 1
Very reactive
- wants to lose electrons
- Reacts spontaniously with O2 and H2O
- Reactions with O2 may create oxides, peroxides, and superoxides
Common uses for Gp 1 Elements?
Na is used in street lights
KCl is used in fertilizer
What makes this element weird?
Lithium
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
What makes this element weird?
Berillium
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
What makes this element weird?
Boron
Group 13
- High melting point, black, hard
- Hydrates are called Boranes
- Very Reactive, wants to complete the octet
- Dimerizes Easily
Describe
Aluminum
Group 13
- Most abundant element in the Earth’s crust
- High thermal and electical conductivity
- Forms covalent compounds with non-metals
- Dimerizes
Describe
Gallium
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
Differences between:
Carbon and Silicon
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
Whats the fancy name for Group 15?
pnicogens
Whats the fancy name for group 16?
chalcogens
What are the two types are phosphorus that we studied?
White and Red
What are the differences between white and red phosphorus?
White
- Waxy, solid
- Toxic
- Low melting point
- Strained
Red
- Solid
- Non-toxic
- High melting point
- Not strained
- Used to make meth
Industrial Applications of Boron
- 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
Where do you find boron and how do you exctract it?
Found in borate minerals, Exctracted by converting then reducing
Oxyacides of Nitrogen
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
Oxyacides of Phosphorus
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
Common Oxides of Nitrogen
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
Oxides of Phosphorus
P4O6
- White, waxy solid
- Formed in reactions with limited O2
P4O10
- White solid
- Formed in reactions with excess O2
Where do you typically find oxygen?
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
Describe
Sulfur
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
Describe
Flurine
Group 17
- The most elecronegative element
- O.N. is allways -1 in compounds
- Never double bonds
Atomic and Physical properites of Group 2
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
Atomic and Physical Properties of Group 18
Nobel Gases
- Unreactive
- Low melting and boiling points
- May create compounds under lab conditions
What are the types of oxides?
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
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
Amphoteric Oxides - properties of both acid and base
- Does not allways react with water
- Includes BeO
- Only react with acids and bases
What makes a good oxidition agent?
Molecules are compounds with elements in high (+) oxidation states
What makes a good reducing agent?
Molecules are compounds with elements in low (-) oxidation states
Does Oxidative power of halogens increase or decrease down the group
Oxidative power decreases down the group
In Group 1 and Group 2, does reducing power increase or decrease down the group
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
What is the oxidation state trends of Gp. 15?
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
Uses for Nitrogen?
- Fertilizer (Made via the Haber Process)
- inert blanketing gas for packaging
- Useful cyrogen
What types of oxydes can alkali metals make?
In exess of oxygen
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
What are the allotopes of carbon?
Carbon, Graphite
* Each C covalently bonded to 3 other C
* Soft, slippery
* Conductive
Diamond
* Giant Covalent
* Has a face-centered cubic (FCC) lattice
* High MP
* Non-conductive
* Very Hard
Carbon “Bucky” Ball or Fullerenes
* Molecular
* Many medical ues (easy to add compounds to)
Carbon Nanotubes
What makes Silicon similar to diamond
- Has an extended structure (or covalent network)
- Has an FCC lattice (like diamond)
- Hard and high MP
SiC (silicon carbide) also has a covalent network and has FCC lattice
