periodic table trends and basics

Question 1

atomic radii trend

Answer 1

• smallest on the right ( bc Zeff increases from left to right - Zeff is the electrostatic pull that the electrons feel bc of the positive charge from the nucleus)
• opposite of all other trends
• size increases going down

Question 2

periodic trends

Answer 2

left to right

• atomic radii decreases
• Zeff increases
• electron affinity increase
• ionization energy increases

Question 3

ionization energy

Answer 3

the energy required to remove one electron from element in the gaseous stage

Question 4

what type of energy removes e-

Answer 4

heat (so always an endothermic reaction)

- need heat to be added, so remove an electron

Question 5

subsequent removal of an electron requires?

Answer 5

more energy - bc there is now more positive/negative

Question 6

characteristic of active metals

Answer 6

low ionization energy ( dont need much to remove e- - bc they want to become nobel gases

Question 7

electron affinity

Answer 7

the energy dissipated by a gaseous species when it gains an electron

• halogens are greedy, want an electron, when they get one, an exothermic reaction happens and expels heat energy

Question 8

removing an electron is a ____ rxn?

Answer 8

endothermic

Question 9

gaining an electron is a _____ rxn?

Answer 9

exothermic

Question 10

electro affinity reported as a pos or neg?

Answer 10

positive in Kj/mol ( but delta H still neg)

Question 11

the stronger the Zeff, the _______ the energy release (electron affinity) when an atom gains an electron

Answer 11

greater

Question 12

atomic mass

Answer 12

mass number = protons and neutrons

Question 13

isotopes

Answer 13

differnt mas numbers, same protons, but different neutrons

Question 14

how many isotops of hyrogen

Answer 14

3; protium, deuterium, tritium

Question 15

energy difference between energy levels is called

Answer 15

quantum - described by planck

Question 16

ml

Answer 16

the particular orbital withing the subshell ( subshell = s, p, d, f) and can be found with 2l + 1 , so for p which is l =1 them ml is 3 –> 3 orbitals

Question 17

electrons fill in order of?

Answer 17

increasing energy ( and electrons further out have the most energy ) 
- if uncertain about filling, use the n +l rule

Question 18

paramagnetic

Answer 18

unpaired electrons –> attracting to magnet

Question 19

diamagnetic

Answer 19

paired electrons—> repelled by magnets

Question 20

where are valence electrons for the transitory elements

Answer 20

s and either d or f

Question 21

where are valence electrons for the representative elements

Answer 21

s and/or p

Question 22

A elements

Answer 22

also called the representative groups 1-8 and have valence in s and/or p

Question 23

B elements

Answer 23

also called nonrepresentative elements (transition elements (s and d) and other below series (s and f) and have valence electrons in the s and either d or f

Question 24

ionic radius and some general rules

Answer 24

• the size of the charged species
• cations (positive- so more pull = smaller)
• anions (negative- less pull- larger)

Question 25

metals

Answer 25

left side and middle

Question 26

nonmetals

Answer 26

right side

Question 27

metals generally _______ electrons to become more -___. and as a result - there ionic radi are ______

Answer 27

loss, positive

- smaller

Question 28

non metals generally ______ electrons and become more _______. and as a result - there ionic radi are ______

Answer 28

gain electrons, negative

• larger

Question 29

alkali metals

Answer 29

1A - have to lose one electron to become nobel gas, low zeff, large radius, like reacting with halogens
- usualy oxidation state of +1

Question 30

alkaline earth metals

Answer 30

+2 oxidation state

Question 31

chalogens

Answer 31

-2 or +6 depending if they are nonmetals or metals
- the group that starts with Oxegen and sulfur
-

Question 32

halogens

Answer 32

-1 ( want to gain one e-), highest electronegativity

Question 33

noble gases

Answer 33

full valence shells - dont want to give up anything- high ionzation energies and virtually non existent e affinities and electronegativity

Question 34

what does high electron affinity mean?

Answer 34

The electron affinity is the energy change when an atom gains electrons. The convention is that the higher or more positive the electron affinity value, the more readily the atom accepts an electron.

Question 35

what does high ionization energy mean?

Answer 35

a HUGE amount of energy is needed to remove and electron ( noble gases have most)

Question 36

why can transition metals form many different colous?

Answer 36

multiple oxidation states