*(DONE/REDO IF TIME)* Chapter 6 - Lecture 7

Question 1

ions (definition and two types)

Answer 1

• Charged atoms formed when electrons are added to or removed from a natural species
• simple ions and polyatomic ions

Question 2

simple ions

Answer 2

• Charged species containing only one atom

Question 3

polyatomic ions

Answer 3

• Charged species containing a group of atoms held together by strong bonds

Question 4

cation (2)

Answer 4

• A positively charged ion

- Result of removing 1 or more electrons from a neutral species

Question 5

anion (2)

Answer 5

• Negatively charged ion

- The result of a natural species gaining one or more electrons

Question 6

atoms

Answer 6

• smallest unit of a substance

Question 7

molecule (2)

Answer 7

• 2 or more atoms that function as a neutral unit

- behaves as an individual unit or particle that defines the substance

Question 8

compounds

Answer 8

• more than one type of atom in the molecule

- h20, CO2, etc.

Question 9

ionic compounds and electron characteristic

Answer 9

• Formed from combinations of anions and cations to give neutral species
• transfer electrons to bond

Question 10

covalent compounds and electron characteristic

Answer 10

• formed from 2 or more non-metals

- share electrons to bond

Question 11

air (definition and 5 components)

Answer 11

• mixture of elements and compounds

- nitrogen, oxygen, hydrogen, carbon dioxide, water vapour

Question 12

at normal atmospheric pressure and room temperature… (3)

Answer 12

• Majority of elements are solids
• 11 are gasses
• 2 are liquids

Question 13

allotropes

Answer 13

• the different structural forms of an element

- example: carbon; diamond, graphite, soot, etc

Question 14

Who made the periodic table? Who updated it?

Answer 14

• Mendelev

- Henry Moseley

Question 15

Metals (3)

Answer 15

• lustre
• thermal and electrical conductivity
• malleability

Question 16

non metals

Answer 16

• absence of metallic properies

Question 17

metalloids

Answer 17

• properties intermediate between those of metals and non metals

Question 18

electron location, movement, and velocity

Answer 18

• outside nucleus
• moves rapidly in a volume that describes the size of the atom
• The greater the velocity of an electron, the higher its energy and the further it can move away from the nucleus

Question 19

what does it mean that electron energy is quantized?

Answer 19

• the energy of an electron is restricted to a certain set of values; therefore, only certain orbits are allowed

Question 20

explain the quantum mechanics model (5)

Answer 20

• The electron does not travel in a circular orbit
• We cannot say where it is at any time but WE can describe the probability of finding it in a defined region
• Energy determines its behaviour about the nucleus
• Energy is quantized (it can only have specific energies)
• Electrons can only have certain specific behaviour

Question 21

electron shells (3)

Answer 21

• the main energy levels
• electrons in the same shell have the same approximate energy and travel abilities
• Max 2n^2 electrons per shell

Question 22

When n (electron shell number) increases… (2)

Answer 22

• Average energy of shell increases

- Distance from the nucleus increases

Question 23

electron subshells (4)

Answer 23

• energy sublevels within an electron shell
• all electrons in the same subshell have the same energy
• # of subshells in a shell= shell number
• labelled by value of n and by letter of specific shell
  (s, p , d, f, g)

Question 24

describe the difference between 1 electron systems and multi electron systems

Answer 24

• 1 electron: subshells within the same shell have the same energy
• multi electron: subshells within the same shell have different energy (s<p></p>

Question 25

energy orbitals

• define
• relate to subshells (2)
• maximum e in each orbital.
• the larger the n…

Answer 25

• Region of space around a nucleus where an electron with a specific energy are most likely to be found
• Have the same energy as the same subshell
• shape and size related to type of subshell
• maximum of 2 electrons in one orbital
• the larger the n, the larger the orbital and energy

Question 26

number of electrons in each shell

Answer 26

2, 8, 18, 32, 50

Question 27

max number of electrons in each subshell

Answer 27

s: 2
p: 6
d: 10
f: 14
g: 18

Question 28

orbital shapes

Answer 28

s: spherical
p: two lobes with 3 different spatial orientations
d: 4 lobes with 5 different spatial orientations/
f: has 7 different spatial orientations

Question 29

number of orbitals in each subshell

Answer 29

s: 1
p: 3
d: 5
f: 7
g: 9

Question 30

aufbau building up principle and hunds rule combined

Answer 30

• electrons fill a set of degenerate orbitals, with one electron in each orbital, all with the same spin, before electrons pair up in an orbital with opposite spins

Question 31

pauli exclusion principle

Answer 31

• two electrons in the same orbital must have opposite spins

Question 32

orbital diagram

Answer 32

• show the electron occupancy of each individual nucleus with arrows to represent electrons