Question 1

electronegativity

Accepted Answer

the ability to attract e- 
-most relavent to covalent cuase the difference in EN determines how e- are shared
If the difference is very large, the more electronegative atom can essentially "take" an electron from the less electronegative atom

Question 2

which element has the highest electronegivity

Accepted Answer

flourine 
(electronegativity increases up and right) 
-excludes nobel gases

Question 3

electron affinity

Accepted Answer

E change that occurs when an atom gains an e- 

also relates to how easily an atom will accept e-. If affinity is ighly negative (Eis released), then the atom "strongly wants" it cause the process is energetically favorable (positive = unfavorable)

Question 4

why would an electron affinity be negitive

Accepted Answer

When an atom gains an electron, it often releases energy (because the atom stabilizes as it gains a more stable electron configuration). This release of energy makes the process exothermic, and therefore, the electron affinity is negative

Question 5

why would an electronegaitivity be positive

Accepted Answer

the process can require E to overcome repulsive forces, like the repulsion between the neg. charged e- being added & the e-s already present around the nucleus. 
-endo process & electron affinity is + (cause E has to be absorbed for the e- to be added).

Question 6

atomic radius

Accepted Answer

the size of the atom 
it is not definite --> it is a probability of its size 
francium has the highest

Question 7

why does size increase as you go down a group

Accepted Answer

it has more electron shells 
more electron-electron repulsion

Question 8

why does size decrease as you move left across a period

Accepted Answer

it has a weaker nuclear charge so the electrons spread out more and are more loosly held (Zeff decreases) 
-the size stays the same

Question 9

units for radii

Accepted Answer

nm or 10^-9 m

Question 10

what happens to the atomic radus when you lose an electron

Accepted Answer

you shrink in size 
losing electrons reverts back to a lower level 
an excess of protons pulls outer electrons closer 
same protons pulling less electrons

Question 11

what happens to the atomic radius when you gain electrons

Accepted Answer

more electron-electron repulsion, so the electrons spread out more and the atom increases in size

Question 12

ionization energy

Accepted Answer

energy needed to remove an electron 
-relative magnitude can be estimated through coulombs law 
further from nucleus = lower IE 
higher nuclear charge = higher IE in a given subshell 
He has the highest 
IE2→ energy to remove the just the second e-

Question 13

levels of ionization energy: highest to lowest

Accepted Answer

filled levels 
filled sublevels

Question 14

explain why removing the 4th electron from Al is drastically harder than removing the 1,2 or 3rd

Accepted Answer

it has 3 valance electrons, so once those were removed,  the fourth had to come from a filled level

Question 15

ground state electron configuration exceptions

Accepted Answer

cr: 4s1 3d5
Cu: 4s1 3d10
Ag: 5s1 4d10 
Au: 6s1 4f14 5d10
why? --> lower E

Question 16

why dont all electrons donate one s electron to a d subshell to gain a full d subshell

Accepted Answer

The cost to move an electron is larger than the stability gained.

Question 17

excited state

Accepted Answer

an electron has absorbed energy and moved to a higher orbital.
Excited states are unstable
Electrons quickly fall back down to the ground state, releasing energy (often as light).
higher energy than the ground state

Question 18

groud state

Accepted Answer

electrons are in the lowest possible energy arrangement.

Question 19

group 1

Accepted Answer

hydrogens and the alkali metals (+1)

Question 20

group 2

Accepted Answer

the alkanlines earth metals

Question 21

group 3-12

Accepted Answer

transition metals

Question 22

group 17

Accepted Answer

the halogens

Question 23

group 18

Accepted Answer

the nobel gases

Question 24

what is the only thing  that affects  Keq

Accepted Answer

temperature
-volume, P, etc, affect it temporarily 
Volume/pressure changes affect concentrations temporarily, not the equilibrium constant itself
ΔG° = −RT ln K     (temperature is in the equation not V or P or M)

Question	Answer
electronegativity	the ability to attract e- -most relavent to covalent cuase the difference in EN determines how e- are shared If the difference is very large, the more electronegative atom can essentially "take" an electron from the less electronegative atom
which element has the highest electronegivity	flourine (electronegativity increases up and right) -excludes nobel gases
electron affinity	E change that occurs when an atom gains an e- also relates to how easily an atom will accept e-. If affinity is ighly negative (Eis released), then the atom "strongly wants" it cause the process is energetically favorable (positive = unfavorable)
why would an electron affinity be negitive	When an atom gains an electron, it often releases energy (because the atom stabilizes as it gains a more stable electron configuration). This release of energy makes the process exothermic, and therefore, the electron affinity is negative
why would an electronegaitivity be positive	the process can require E to overcome repulsive forces, like the repulsion between the neg. charged e- being added & the e-s already present around the nucleus. -endo process & electron affinity is + (cause E has to be absorbed for the e- to be added).
atomic radius	the size of the atom it is not definite --> it is a probability of its size francium has the highest
why does size increase as you go down a group	it has more electron shells more electron-electron repulsion
why does size decrease as you move left across a period	it has a weaker nuclear charge so the electrons spread out more and are more loosly held (Zeff decreases) -the size stays the same
units for radii	nm or 10^-9 m
what happens to the atomic radus when you lose an electron	you shrink in size losing electrons reverts back to a lower level an excess of protons pulls outer electrons closer same protons pulling less electrons
what happens to the atomic radius when you gain electrons	more electron-electron repulsion, so the electrons spread out more and the atom increases in size
ionization energy	energy needed to remove an electron -relative magnitude can be estimated through coulombs law further from nucleus = lower IE higher nuclear charge = higher IE in a given subshell He has the highest IE2→ energy to remove the just the second e-
levels of ionization energy: highest to lowest	filled levels filled sublevels
explain why removing the 4th electron from Al is drastically harder than removing the 1,2 or 3rd	it has 3 valance electrons, so once those were removed, the fourth had to come from a filled level
ground state electron configuration exceptions	cr: 4s1 3d5 Cu: 4s1 3d10 Ag: 5s1 4d10 Au: 6s1 4f14 5d10 why? --> lower E
why dont all electrons donate one s electron to a d subshell to gain a full d subshell	The cost to move an electron is larger than the stability gained.
excited state	an electron has absorbed energy and moved to a higher orbital. Excited states are unstable Electrons quickly fall back down to the ground state, releasing energy (often as light). higher energy than the ground state
groud state	electrons are in the lowest possible energy arrangement.
group 1	hydrogens and the alkali metals (+1)
group 2	the alkanlines earth metals
group 3-12	transition metals
group 17	the halogens
group 18	the nobel gases
what is the only thing that affects Keq	temperature -volume, P, etc, affect it temporarily Volume/pressure changes affect concentrations temporarily, not the equilibrium constant itself ΔG° = −RT ln K (temperature is in the equation not V or P or M)

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Chem Study Guide 1