chp 2 general chem DAT

Question 1

atomic symbols -

Question 2

left bottom number

Answer 2

protons

Question 3

left top number

Answer 3

atomic mass

Question 4

atomic mass =

Answer 4

protons + neutrons

Question 5

neutrons =

Answer 5

atomic mass - protons

Question 6

electrons =

Answer 6

protons = electrons
unless element has a charge then sub or add the charge

Question 7

bohr model of the atom

Answer 7

1913 Niels Bohr created the first working model of hydrogen atom

• as energy moves up the next shell , the shell gets smaller and further from the nucleus

Question 8

what is quantization ?

Answer 8

the concept that a physical quantity, like energy, can only exist in discrete, specific values

Question 9

what are electrons ?

Answer 9

they zoom through 3D atomic or molecular orbitals

Question 10

4 types of orbital

Answer 10

S,P,D,F

Question 11

s orbital

Answer 11

shaped like spheres. not 2D circle. low energy orbitals are buried inside the higher energy orbitals

Question 12

p orbitals

Answer 12

shaped like dumbbells. each energy level has 3 p orbitals (horizontal, vertical and diagonal )

when we say 2p shell we refer to 3 separate p orbitals

Question 13

d orbitals

Answer 13

looks like a 4 leaf clover. there are 5 diff d orbitals per shell.

Question 14

transition metals

Answer 14

are bright colored because they have a funky d orbital shaped that allows electrons in the d orbitals to absorb colored light and promote higher energy orbitals within d shell

Question 15

f orbitals

Answer 15

they have 7 diff shapes.

Question 16

s block

Answer 16

2 columns wide. 1 s orbital per shell

Question 17

f block

Answer 17

14 column wide, 7 f orbitals per shell

Question 18

d block

Answer 18

10 columns wide. 5 d orbitals per shell

Question 19

f block

Answer 19

6 columns wide . 3 f orbitals per shell

Question 20

principle - quantum number

Answer 20

1,2,3,4=n
this tells us in which shell the electron is in or how far its from the nucleus

Question 21

azimuthal - quantum number

Answer 21

L = 0,1,2,3
tell us in which orbital the electron is in
0,1,2,3->s,p,d,f

Question 22

magnetic -quantum number

Answer 22

m = neg to pos number
tells us in which p orbital , d orbital or f orbital electron Is in

ex if its in p orbital, they only have 3 diff orbitals so -1,0,1

Question 23

ms -quantum number

Answer 23

spin number
equal to -1/2 or 1/2

Question 24

what does electron conf mean ?

Answer 24

description of quantum numbers and orbitals

Question 25

1s2

Answer 25

1= is the principal quant number or energy n=1

s = what kind of orbital these electrons are in s means L = 0

2 = shows how many electrons are in the orbital

Question 26

oxygen ex electron conf

Answer 26

1s22s22p4

2p4 means there are 4 electron using the 3 p orbitals ( 3 p because there are 3 p orbital types )

Question 27

hunds rule

Answer 27

electrons never pair up unless there is no more space

Question 28

condense electron conf

Answer 28

you write the noble gas before the element and the rest of the electron conf

Question 29

bromine condense conf

Answer 29

Ar-4s23d104p5

Question 30

valance vs core electrons

Answer 30

valence e are the ones in the outermost shell and core e are inside the inner shells.

Question 31

valence electrons

Answer 31

the ones with the largest Principle quantum number

Question 32

exception for valence electrons

Answer 32

elements in the d block , d shell electrons are also valence.

Question 33

atomic orbital energy diagram

Answer 33

the larger the electrons principle quantum number the further away from the nucleus it is and higher in energy

Question 34

rules for e-

Answer 34

aufbau: electrons fill the lowest energy orbitals firs

hunds ; electron don’t pair up until they have to

pauli ; no 2 electrons in the same atom can have the same quantum number

Question 35

excited vs ground state

Answer 35

ground state is the normal regular state

excited state is when an electron absorbs a photon of light which get promoted into a higher energy shell

when a electron falls back to ground state it emits color

Question 36

paramagnetic vs diamagnetic

Answer 36

paramagnetic = unpaired electrons - which makes them attracted to magnets
(ODD number of e)

diamagnetic = all electrons are paired - they slightly resell magnetic fields (ODD or EVEN number of e)

Question 37

a photons energy

Answer 37

the particle of light (photon)can be calculated using
Ephoton = hf=hc/wavelenght

Question 38

photons energy

Answer 38

as energy increases , frequency increases = wavelength decreases

Question 39

photoelectric effet to function …

Answer 39

metal has to be hit with a photon with enough energy. ( photon must have high frequency and low wavelength )