Chemistry Chapter 1 Atomic Structure

Front 1

which atoms are found within the nucleus of an atom

Back 1

protons and neutrons

Front 2

charge of a proton/electron?

Back 2

1.6e-19Coulombs

Front 3

atomic number(Z)

Back 3

Protons

Front 4

Mass number(A)

Back 4

Protons + Neutrons

Front 5

structure of Element from the periodic table? X^(?)_?

Back 5

X^A_Z
where A is the superscript
Z is the subscript

Front 6

isotope

Back 6

same proton#, different Neutron number

Front 7

electron <<< proton in mass

Back 7

know this

Front 8

lower electric potential of electron =

Back 8

closer to nucleus

Front 9

higher electric potential of electron =

Back 9

further from the nucleus

Front 10

trend: further from nucleus = higher energy level

Back 10

know this

Front 11

outer shell electrons that feel the least electrostatic pull towards the nucleus are _____

Back 11

valence electrons
-more likely to become involved in bonds with other atoms

Front 12

valence electrons determine the _____ of an atom

Back 12

reactivity

Front 13

neutral state of an atom =

Back 13

equal number of electrons and protons

Front 14

gain of electrons is _____

Back 14

negative charge; anion

Front 15

loss of electrons is ______

Back 15

positive charge; cation

Front 16

electrons are found ____ the nucleus in separate but defined ______

Back 16

outside; shells or orbitals

Front 17

determine the number of protons, electrons and neutrons in Ni

Back 17

P: 28
N: 30
E: 28

Front 18

atomic mass

Back 18

aka the mass number (P + N)

Front 19

atomic weight

Back 19

g/mol
-look off the periodic table

Front 20

avogadro's number

Back 20

6.02e23

Front 21

isotopes of Hydrogen

Back 21

hydrogen/protium = 1P, 1E, 0N
deuterium = 1P, 1E, 1N
tritium = 1P, 1E, 2N

Front 22

energy equation

Back 22

E =hf

E = joules
f = frequency
h = 6.6e-34J*s

Front 23

Bohr model of hydrogen
angular momentum =
energy of the electron =

Back 23

L = nh/2(pi)

n = quantum number
h = 6.6e-34

E = -Rh/n^2

Rh = 2.2e-18
n = quantum number

Front 24

trend within angular momentum equation?

Back 24

yes;

L ~ n since (h/2(pi)) is a constant

Front 25

trend with energy of the electron equation?

Back 25

yes

E ~ 1/n^2
so as one goes up in quantum numbers(n) the energy is drastically increased since the E value approaches "0" which is getting larger

Front 26

orbit with the smallest radius around the nucleus is the ______ state which corresponds to n = ?

Back 26

ground state
n = 1

Front 27

excited state

Back 27

n > 1

Front 28

electrons can obtain an excited state through ______

Back 28

use of heat
use of radiation

Front 29

excited --> ground = ____

Back 29

emission of light/energy

Front 30

ground --> excited = _____

Back 30

absorption of light/energy

Front 31

emission of light occurs in _____ amounts of energy in the form of ______

Back 31

discrete/pre-determined
photons

Front 32

electromagnetic energy equation
E =

Back 32

E = hc/lambda

h = 6.6e-34
c = 3e8
lambda = wavelength (e-9)

Front 33

trend within the electromagnetic equation?

Back 33

yes;
E ~ 1/lambda; as lambda becomes larger(800nm) the Energy level decreases

as lambda becomes smaller(closer to 0) the energy value increases

this is in relation to frequency;
higher frequencies produce smaller wavelengths thus higher energy outputs!

Front 34

emitted wavelength ~ to energy transition experienced

Back 34

know this

Front 35

Bohr + Planck theory EQ
E = hc/lambda = -Rh(Ni^-2 - Nf^-2)

Back 35

know this

Front 36

trend with bohr/planck theory?

Back 36

yes; energy is proportional to frequency (inversely to lambda)

this means that the larger the difference between Ni^-2 - Nf^-2 is, the larger the energy will be

ex) 1 --> 2 vs 1 --> 4
1-->2 will be smaller in energy than 1-->4

Front 37

electrons move within ____ around the nucleus

Back 37

orbitals

Front 38

heisenberg uncertainty principle

Back 38

can not determine position and momentum at the same time

momentum = p = mv
can determine momentum and velocity though!

Front 39

quantum numbers(4)

Back 39

n, l, M(l), M(s)

Front 40

principal quantum number

-max number of electrons?

Back 40

= n
associated with valence shell energy level and radius size

max number = 2n^2

Front 41

difference in energy between energy levels(n)....

Back 41

decreases with increased n value

ex) 1-->2 vs 3-->4
using 1/Ni^2 - 1/Nf^2

=1 - .25 = .75
= .111 - .0625 = .04861

Front 42

azimuthal number

max number?

Back 42

= l
the number of subshells within an energy level

max number is 4l + 2

Front 43

range of (l) values?

Back 43

0 to n-1

Front 44

magnetic number

Back 44

= M(l)
orbital within the subshell

Front 45

values for M(l)

Back 45

-l to l

Front 46

M(l) values of:
s -->
p -->
d --->
f --->

Back 46

s = 0
p = -1,0,1
d = -2,-1,0,1,2
f = -3,-2,-1,0,1,2,3

Front 47

s shell =
p shell =

Back 47

spherical
dumbbell
p orbitals broken into Px,Py,Pz

Front 48

spin number

Back 48

= M(s)
+ 1/2
- 1/2

Front 49

if two electrons are in the same orbital, they must have ____ spins

Back 49

opposite

Front 50

electrons in different orbitals but same M(s) values are in _____

Back 50

parallel

Front 51

orbitals are filled

Back 51

low to high energy

Front 52

show the pattern of filling for the element Carbon

Back 52

1s2 /2s2/ 2p2

Front 53

what orbital in n = 3 has the largest energy?

Back 53

3d...dont forget that this is part of n = 3!!!

Front 54

to gain/lose a charge, what is manipulated?

Back 54

electrons

Front 55

hunds rule

Back 55

orbitals are filled until all are filled
(either not full, half full or completely full)

Front 56

what is the exception to metal cations within the d shell?

Back 56

they will lose their s electrons before they lose their d electrons

Front 57

what are two elements within the d shell that fill weirdly?

Back 57

Mn and Te
Mn+ = [Ar]4s1,3d5
Te+ = [Kr]5s1, 4d5

Front 58

paramagnetic

Back 58

unpaired electrons; weakly attracted to magnetic field

Front 59

diamagnetic

Back 59

all paired electrons; repelled by magnetic field
ex) Be = 1s2, 2s2
elements on the right side of the table

Front 60

valence electrons

Back 60

outermost electrons