chapter 5 Flashcards
1
Q
explain electron shells
A
- they are energy levels, each shell has a different quanta number
- as the number of the shell increases, the energy of the electron increases
- electrons can only exist at specific quantum levels
- energy levels get closer together as the energy increases
2
Q
what are atomic orbitals
A
- they are regions of space around the nucleus of the atom that can hold up to 2 oppositely spinning electrons
3
Q
describe s orbitals
A
- they are a spherical shape
- every shell from n=1 has them
- the greater the shell number, the greater the radius of the s orbital
4
Q
describe the p orbital
A
- dumbbell shape
- ever shell from n=2 has them
- the greater the shell number, the further away the p orbital is
5
Q
describe d orbitals
A
- every shell from n=3 has them
- there are 5 d orbitals
6
Q
describe f orbitals
A
- every shell from n=4 has them
- there are 7 f orbitals
7
Q
describe subshells
A
- a new type of atomic orbital is added for each new electron
- orbitals of the same type are grouped together as subshells
8
Q
what is ionic bonding
A
- the strong electrostatic forces of attraction between oppositely charged ions
9
Q
explain the structure of ionic compounds
A
- they are held in a giant ionic lattice
- each ion exerts electrostatic attraction in all directions
- they are closely packed in a repeating pattern
10
Q
explain the melting and boiling point of ionic compounds
A
- generally have high melting and boiling points
- they are solids at room temperature
- the electrostatic attraction between the ions are strong
- a large amount of energy is required to overcome these forces
- it also depends on the size of the ions and the atomic charge
11
Q
describe the solubility of ionic compounds
A
- many ionic compounds dissolve in polar substances
12
Q
describe the electrical conductivity of ionic compounds in the solid state
A
- the ions are held together in a fixed lattice
- the ions are not free to move meaning there are no mobile charge carriers
- there is no electrical conductivity
13
Q
explain electrical conductivity of ionic compounds in the molten state
A
- the ions are free to move
- there are mobile charge carriers
- electricity is conducted
14
Q
what is the definition of an element
A
- a substance made up of only one type of atom
15
Q
what is a compound
A
- a substance consisting of two or more elements chemically bonded together
16
Q
what is a molecule
A
- a group of atoms covalently bonded together
17
Q
what is covalent bonding
A
- strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms
- it is the overlap of atomic orbitals
- they are localised = the attraction is only between the nuclei and the pair of electrons of the bonded atoms
18
Q
what is a dative covalent bond
A
- a shared pair of electrons in which the bonded pair has been provided by one of the bonded atoms only
- shown as an arrow of the displayed formula
19
Q
what is bond enthalpy
A
- it serves as a measurement of covalent bond strength
- as the strength of the bond increases, the bond enthalpy value will increase
