Periodicity

Question 1

Ferromagnetic

Answer 1

Cobalt
Iron 
Nickel 
(HIGHEST) 
- because they have all unpaired electrons and want to bond)

Question 2

Ligands

Answer 2

atoms or ions which possess lone pairs of electrons to form co-ordinate bonds to the central ion and donate a lone pair to a vacant orbital

Question 3

Colorimetry

Answer 3

a change of ligand can change the color of the compound

Question 4

Dative (Coordinate bond covalent)

Answer 4

when the electrons shared in a bond is coming from only one atom

Question 5

Color depends on…

Answer 5

Oxidation state
Transition element
Ligand
Coordination Number

Question 6

Multidentate

Answer 6

can form several co-ordinate bonds/dative bonds

Question 7

diamagnetic

Answer 7

LOWEST

Least amount of unpaired electrons in the shell

Question 8

paramagnetic

Answer 8

anything with lone electrons or half filled

Question 9

Unidentate

Answer 9

ligands that bond once or give one electron

Question 10

List of ligands

Answer 10

Chloride 
Cyanide
Hydroxide
Oxide
Water
Ammonia

Question 11

Atomic size trend

Answer 11

Group: Increases (more energy levels)
Period: Decreases (more protns pulling closer)

Question 12

Variable oxidation states

Answer 12

arises from the similar energies required from removal of 4s and 3d electrons

Question 13

Electron Affinity

Answer 13

Period: Increases (atoms are smaller and there is a greater charge)
Group: Decreases (atoms get bigger and there are more shells)

Question 14

IOnic Radius

Answer 14

Cations are formed by losing electrons (smaller = metals) and anions are formed by gaining electrons, these electrons then createe an ionic bind and are shared between the two anion and cation

Question 15

Electron Affinity

Answer 15

Energy change associated with adding a mole of electrons to a mole of gaseous atoms

Question 16

IOnization Energy Trend

Answer 16

Group: Decreases ( there is greater distance and more shielding)
Period: Increases (greater nuclear charge)

Question 17

HIGHER ionization energy IF …

Answer 17

There are filled or half filled orbitals

Question 18

Ionization Energy

Answer 18

Amount of energy required to completely remove a mole of electrons from a mole of gaseous atoms

Question 19

Transition Element metallic properties

Answer 19

• Strong metallic bonds due to the small ionic size and close packaging
• higher melting point
• higher boiling point

Question 20

IOnic Radius Trend

Answer 20

Group: Increases
Period: Decreases then increases then decreases

Question 21

Melting and boiling point trends

Answer 21

• Period: rises to a mzaximum near the middle of the period and then falls off at a minimum value at the end of the period
• Group: Increases from top to bottom (increase in atomic #)
• Alkali and Metalloids: decrease with increasing atomic number
  As the atomic # increases, MP and BP increases because there are more electrons whoch creates a larger negative charge around the nucleus of the atom

Question 22

Boiling POint

Answer 22

The temperature which the vapor pressure of a liquid is equal to the external pressure of the liquid

Question 23

Isoelectric Ions

Answer 23

Ions with the same number of electrons. The one with the greater charge has the smaller atomic radius

Question 24

Electronegativity Trend

Answer 24

Group: decreases
Period: Increases

Question 25

Electronegativity Def

Answer 25

Tendencey for an atom to attract in ion to itself when it’s chemically combined with another element

Question 26

Melting POint

Answer 26

the temperature at which the crystal lattice of a solid collapses and the solid is converted into a lqiuid