Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem 101 > Main Group Chemistry > Flashcards

Main Group Chemistry Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Physics 101 flashcards Psychology 101 flashcards Chemistry 101 flashcards AP® Chemistry flashcards Biology 101 flashcards Organic Chemistry 101 flashcards Sociology 101 flashcards
1
Q

What is the difference between second and third period elements

A

The second period elements are often anomalous in their behaviour, whereas the third period elements are more representative of the group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Why do 2nd period elements have anomalous behaviour

A
  1. Small size and high electronegativity
  2. Maximum of four covalent bonds (no d orbitals for bonding)
  3. More common occurrence of multiple bonding (good pi overlap of 2p orbitals)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What happens proceeding down a group

A

Metallic behaviour increases, positive oxidation states are prevalent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

True or false: all halogens can form only one oxidation state (-1)

A

False. Only fluorine forms (-1) oxidation state because it is the most electronegative Halogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Why are expanded octets and corresponding hybridization not observed in 2nd row elements

A

Because valance orbitals of 2nd row elements are restricted to 2s and 2p orbitals and only hybridization scheme is restricted to four covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Why is it more common to see multiple bonding in 2nd row elements than 3rd row and beyond?

A

Because in 2nd period elements the 2p orbitals are closer in proximity to each other which makes pi bonding more effective

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Properties of alkali metals

A
  • unusually soft
  • have lower melting/boiling points & densities

*this is because of their large ionic size and ns^1 valence electron configuration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Why are crystal structures easily deformed in alkali metals

A

The single valence e- is not held tightly and the metallic bonding in the solid is weak

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Are alkali metals good reducing or oxidizing agents

A

Powerful reducing agents

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Properties of alkali earth metals

A

Harder & higher melting than alkali metals, somewhat less reactive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the use of alkali earth compound CaCO3

A

Calcium carbonate is heated to obtain calcium oxide (lime)

Has essential roles in steel making, water treatment, used to make glass, whiten paper, and neutralize acidic soil

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is unique about BE

A
  • unreactive in air and water
  • BeO is an amphoteric oxide
  • have strong covalent character and conduct electricity poorly
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Why is gallium smaller than aluminum

A

Because of the presence of an intervening 3D sub shell, which increases Zeff

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are properties of boron

A
  • metalloid with a covalent network structure

- black, hard, high mp

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is the molecular formula of boron

A

B2H6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What are common applications of boron

A

Pyrex glass, sodium perforate as colour safe bleach, and boric acid as cockroach insecticide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What does the three-center-two-electron bond illustrate

A

The electrons can be delocalized over more than two atoms

18
Q

What is the major ore of aluminum and how is it extracted

A

Bauxite (Al2O3)

Converting Al2O3 to Al takes place through a reduction process followed through by electrolysis

19
Q

What are applications of aluminium

A

Aluminium forms alloys that are strong & light weight & resistant to corrosion.

Aircraft, bicycles, appliances

20
Q

What are pnictogens

A

Group 15 elements

21
Q

What do nitrogen and phosphorus do

A

Combine with many non-metals to form covalent compounds and attain oxidation states from -3 to +5

22
Q

What is nitrogen used as

A

A cryogen, (low temp refrigerant) to store temp sensitive samples

23
Q

What is white phosphorous

A

An allotrope of phosphorus

White, waxy, highly toxic solid with a low melting point (44c) and glows faintly

Narrow bond angles are incompatible with any localized bonding scheme so it is highly reactive

24
Q

What is red phosphorus

A

Red, non-toxic solid with a high melting point

Bonds are not strained so it is less reactive than white phosphorous. Used to manufacture meth

25
Q

How do you extract phosphate from phosphate rock ( Ca3(PO4)2)

A

Reduction process with the use of carbon as a reducing agent

26
Q

Properties of NH3 (ammonia)

A

Colourless gas

Prepared by barber process

Used as fertilizer & base

27
Q

Properties of PH3 (phosphine)

A

Extremely toxic gas

Weaker base than NH3

28
Q

Properties of N2O

A

Dinitrogen Monoxide

  • colourless, sweet smelling gas
  • dental anesthetic (laughing gas)
  • propellant for whipped cream
29
Q

Properties of NO(g)

A

Nitrogen monoxide

Colourless, paramagnetic gas
Air pollutant, neutral transmitter

30
Q

Properties of NO2

A

Nitrogen dioxide

Brown, toxic gas; implicated in photochemical smog

Formed by reaction of NO + O2

31
Q

How is phosphorous trioxide formed

A

P4O6

P4(s) + limited O2(g) -> P4O6(s)

32
Q

How is phosphorus pentoxide formed

A

P4O10

P4(s) + excess O2(g) -> P4O10(s)

33
Q

Draw Lewis structures for

A

Nitrous acid

Nitric acid

Phosphorous acid

Phosphoric acid

34
Q

Nitrous acid

A

HNO2
-weak acid
+3 oxidation state

Conjugate base is NO2-

35
Q

Nitric Acid

A

HNO3

  • strong acid
  • N atom in +5 oxidation state
  • major application is to form ammonium nitrate (fertilizer)
  • very strong oxidizing agent
36
Q

Phosphorous acid

A

H3PO3

  • weak acid
  • P atom in +3 oxidation state
  • diprotic acid
37
Q

Phosphoric acid

A

H3PO4

  • weak acid
  • P atom in +5 oxidation state
  • tripotic acid
  • main application is starting material for fertilizers
38
Q

What is a diprotic acid

A

One of the H atoms is directly bonded to the central P atom and is not acidic

39
Q

What is a triprotic acid

A

Three acidic H atoms that could potentially dissociate

40
Q

Properties of O2

A

Dioxygen

-colourless, paramagnetic gas

41
Q

Properties of O3

A

Ozone

-bluish, pungent, diamagnetic

Chem 101 (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions