Chem Subject Test 1 And 2 "atomic Structure"

Front 1

atomic number (Z)

Back 1

# of proton

z=bottom

Front 2

mass number (A)

Back 2

number of proton and neutron

A = top

Front 3

isotopes

Back 3

atom with same atomic number but different mass number
(same proton different neutron)
btw isotopes same chemical characteristic but different physical characteristic

Front 4

mole

Back 4

the amount of a substance that contains the same number of particles as there are atoms in 12 g of 12C

1 mole = 6.022x10^23 particles
(avagadro's number)

Front 5

avagadro's number

Back 5

6.022X10^23 particles

Front 6

Bohr's model of the atom

Back 6

protron and neutron in the center and electron movining around the center

microsocopic solar system

Front 7

quantum mechanical model

Back 7

P and N in the center and
electron clouds

Front 8

plank's theory

Back 8

E=hf = hc/ㅅ

ㅅ= wavelength
f= frequency
h=plank's constent

Front 9

quantum numbers

Back 9

principle quantum number (n)

azimuthal quantum number (l)

magnetic quantum number (ml)

spin quantum number (ms)

Front 10

Principle quantum number (n)

Back 10

energy shell, can have value of 1,2,3 ect

give overall E. level, size of e- path

as n inc =radius inc = higher energy level

전자의 에너지 상태와전자 구름모양 및 방향성을 나타냄

maximum # of e- per shell is 2n^2

Front 11

which quantum number affects the energy of orbit

Back 11

n and l

Front 12

azimuthal quantum number (l)

Back 12

subshell; values from 0 -> n-1

(s,p,d,f = 0,1,2,3)=different orbital in same subshell

large the l, higher the energy of subshell

Front 13

n+l rule

Back 13

smaller value of n+l then the orbital will be lower in energy

Front 14

magnetic quantum number (ml)

Back 14

describe the orientation of the orbital in space

if l =1 then ml is -1,0,1

ml divides subshell into individual orbital and defines the orientation of the orbital

ml does not affect the energy of the orbital only dictates the orentation thus
px, py, pz equal in energy

Front 15

the maximum # of e- per shell is ?

Back 15

2n^2

Front 16

the maximum number of e- inany subshell is ?

Back 16

4l+2

Front 17

any value of l , what is possible value of ml

Back 17

2l+1

Front 18

spin quantum number

Back 18

only one of two values
+1/2 and -1/2

no effects on energy or orbit

Front 19

Heisenberg uncertainty principle

Back 19

it is impossible to determine with complete accuracy both the position and the momemtum of an e- simultaneously

Front 20

pauli's exclusion principle

Back 20

no two electrons in an atom can have the same four quantum numbers (n,l,ml,ms)

Front 21

electron configuration

Back 21

order of filling
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d

Front 22

valence e-

Back 22

the e- that are not included in the inner shell, comprise the outer shell

[Ne]3s^3 3p^3

Front 23

n+l rule in configurarion

Back 23

subshell with lower (n+l) fill first

if the n+l sums of two subshell are equal the lower n subshell will fill first

ex 4s, n+l=4 and 3d, n+l=5
thus 4s fill first

Front 24

Hund's rule

Back 24

states that with a given subshell, orbitals are filled such that there are maximum number of half filled orbitals with parrllel spins

Front 25

paramagnetism

Back 25

has unpaired electron and drwaned into magnetic field

Front 26

diamagnetism

Back 26

no unpaired electron

Front 27

the periodic table trand

Back 27

from left to right
-electronegativity inc
-ionization energy inc
-atomic radius dec

from bottom to top
-electronegativity inc
-ionization energy inc
-atomic radius dec

Front 28

period in periodic table

Back 28

row (from left to right)

Front 29

column in periodic table

Back 29

group of family (top-bottom)

same characteristic due to same valence e-

Front 30

aufbau principle

Back 30

building up principle

e-fill in the lowest energy orbital first

Front 31

Atomic radius

Back 31

indication of the size of the atom

metal A.R> cation(+ ion) radius

nonmetal A.R< anion (- ion) radius

A.R 크면 가장 바깥에 전자 껍질의 잔자는 쉽게 덜어저 나가 cation 이 되기쉽고

A.R 작으면 전자를 얻기쉬워 anion이 되기쉽다

Front 32

electronegativity

Back 32

measure of of the attraction an atom has for electron in a chemical bond.

how long an atom holds onto its e-

Front 33

ionization energy

Back 33

the energy required to completely remove an elctron from an tion or ion

Front 34

electron affinity

Back 34

the energy released when an electron is added to a gaseous atom

Front 35

metal

Back 35

electropositive
have tendency to lose e-

ductile
shiny solid
high M.P and density

low ionization, electronegativity

high atomic radius

thus valence e- can move freely

maileability (deformed w/o breaking)

Hint 35

p.t far left side

Front 36

transistion metal

Back 36

form cantion

XXX e- is moved from s orbital before they are removed from d orbital

ex Mn= [Ar]4s^2 3d^5
Mm^2+ =[Ar]3d^5

high M.P and B.P

formed high colored solution in ionic form

Hint 36

p.t in the middle

Front 37

nonmetal

Back 37

high ionization, electronegative

low A.R

poor conductor of heat and electricity

gain e- easily (anion)

brittle in solid state

Front 38

metalloids

Back 38

semi metal

have both metal and nonmetal characteristics

Front 39

equation needed to calulate the energy emitted when an electron relaxed from n=3 to n=2

Back 39

E= Rh(1/Ni^2=1/Nf^2)

Rh is given

Front 40

equation used to determine which of the principle energy levels has an energy of -328KJ/mol

Back 40

E=-Rh/n^2

Front 41

what is group O

Back 41

nobel gas

Front 42

what is group IVB

Back 42

Roman numeral represents the number of electrons what will lie outside the noble gas core configuration

letter A and B tells wheather atom is representitive or nonrepresentitive

representitive fill S and P block

non representitive fill s, d and maybe f orbtal

Front 43

positive ion's will have () radii than the corresponding neutral atoms and greater the positive charge the ()the ionic radius

Back 43

smaller

smaller

Front 44

negative ions will have () radii than the corresponding neutral atoms and greater the negative charge () ionic radious

Back 44

greater

greater

Front 45

negative ion O^2-

Back 45

electron 이 neutral state 보다 2개 더 많다. 2개를 빼야지 원래 neutral state가 됀다

thus atomic radi of anion is greater than neutural state

Front 46

positive ion K+

Back 46

neutral state 보다 e- 이 없다
하나를 더해야지 neutral state가됀다

e-을 일어버렸기때문에 neutral state 보다 radius가 더 작다

Front 47

which of the following have greater atomic radius

Ca+2 and Ar

Back 47

same e- number but Ca has more proton thus greater electronegativity and smaller radius.

Front 48

same chemical characteristic but different physical characeristic

Back 48

isotope