Transition Metals

Front 1

trend of atomic size as you move down a column in the periodic table (for main group elements)

Back 1

- atoms increase their size because outermost principal energy energy level increases (larger orbitals)

Front 2

trend of atomic size as you move across a row in the periodic table (for main group elements)

Back 2

- atoms decrease their size because there is stronger attraction between outermost electrons and nucleus

Front 3

trend of atomic size as you move across a row in the periodic table (for transition metals)

Back 3

- first two elements decreases, but fairly constant radius because the additional electron goes into a lower orbital (n-1), which makes the atom experience a constant effective nuclear charge

Front 4

trend of atomic size as you go down a group in the periodic table (for transition metals)

Back 4

-small but expected increase in atomic size (1st and 2nd row of transition metals)

Hint 4

-almost constant for 2nd and 3rd row of transition metals

Front 5

lanthanide contraction

Back 5

14 out of 32 electrons go to the (n-2)f sublevel, which have lower principal quantum levels (not effective in shielding the outer electrons from nuclear charge)

Hint 5

-electrons in the outermost orbital are attracted more to the nucleus, making increase in atomic size less evident.

Front 6

define: ionization energy

Back 6

energy required to remove an electron from the atom or ion in the gaseous state

Front 7

trend in ionization energy as you go down a column in the periodic table (main group)

Back 7

-IE decreases because principal quantum number increases; electrons are further away from the nucleus, making it easy to strip them from the atoms

Front 8

trend in ionization energy as you move across a row (main group)

Back 8

IE increases because atoms experience a greater effective nuclear charge; electrons are held more tightly making it more difficult to strip them away from the atom.

Front 9

trends in IE when moving across a row in the periodic table (for transition metals)

Back 9

slight increase in a row because of atomic size

Front 10

trends in IE when moving down a column in the periodic table (for transition metals)

Back 10

slight decrease down a column, but an increase in the third row, because atomic radius in the third row is almost similar to that of the second row --> electrons are held more closely.

Front 11

define: electronegativity

Back 11

ability of an atom to attract electrons in itself in a chemical bond

Front 12

trends in electronegativity when moving across a row in the periodic table (for main group)

Back 12

increases across a period --> AR is smaller and nucleus gets more positive as we move across a column

Front 13

trend in electronegativity when moving down a column in the periodic table (for main group)

Back 13

decreases down a period -> AR is bigger, more distance from the nucleus to the electron of the other atom

Front 14

trend in electronegativity when moving across a row in the periodic table (for transition metals)

Back 14

SLOWLY increase in a row --> slight increase in atomic radius, and nucleus is becoming more positive

Front 15

trend in electronegativity when moving down a column in the periodic table (for transition metals)

Back 15

increase in first to second row, because nucleus becomes more positive and the AR is nearly constant, wanting to draw electrons to itself
- no change in 2nd and 3rd row

Front 16

define: ligand

Back 16

Lewis base that donates an electron pair to the transition metal

Front 17

define: complex ion

Back 17

central metal ion bound to one or more ligands

Front 18

define: coordination compound

Back 18

complex ion bonded to a counterion

Front 19

define: monodentate ligands

Back 19

ligands that donate only one pair of electron pair to the central metal

Front 20

define: bidentate ligands

Back 20

ligands that donate two pairs of electrons to the central metal

Front 21

define crystal field splitting energy

Back 21

energy difference between a set of d orbitals

Front 22

define a low-spin complex

Back 22

-d electrons are placed in the lower energy d orbitals and are paired

Hint 22

-energy difference is large

Front 23

define a high-spin complex

Back 23

-electrons are placed in both the higher and lower energy orbitals before any pairing occurs

Hint 23

-energy difference is small

Front 24

properties in the energy diagram to make a complex solution transmit/absorb color

Back 24

d electrons must be present, and there must be vacant d orbitals or d orbitals containing only one electron.

Front 25

define diamagnetic substances

Back 25

contain no net electron spin and are repelled from a magnetic field.

Hint 25

will be pushed up, away from the magnetic field in a Guoy balance (decreasing its apparent mass)

Front 26

define paramagnetic substances

Back 26

contain one or more unpaired electrons and are attracted to a magnetic field.

Hint 26

will be pulled down toward the magnetic field in a Guoy balance increasing its apparent mass

Front 27

exceptions in trend in orbital filling for transition metals

Back 27

- Nb, Mo, Ru, Rh and Ag result in a 5s^1d^x configuration and Pd results in a [Kr]4d^10 configuration.