Chem Exam 1

Question 1

Quantum Numbers

Answer 1

tell us where to find electron in an atom (orbital and spin)

Question 2

Principle Quantum Number

Answer 2

symbol: n
tells us the electrons energy level
the bigger the n value, the higher the energy level

Question 3

Azimuthal Quantum Number

Answer 3

symbol (L)
Shape of the space where we might find electron

Question 4

Magnetic Quantum #

Answer 4

symbol (ml)
Tells you orientation of orbital
when L = 0 there is only one possible orientation for

Question 5

Spin Quantum #

Answer 5

(ms)
tells you the spin (up or down)

Question 6

Electron Configuration

Answer 6

how electrons fill up the orbitals

Question 7

Aufbau Principle

Answer 7

rule book for how electron configuration is filled
–> fill orbitals in order of increasing energy

Question 8

Hund’s Rule

Answer 8

when filling up orbitals that have the same energy level, they will each occupy their own before doubling up

Question 9

orbitals

Answer 9

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

Question 10

Element Written

Answer 10

X = element
A = atomic mass #
Z = atomic #

Question 11

Mass measured in

Answer 11

grams (g)

Question 12

Volume measured in

Answer 12

liter (L) or cubic centimeter (cm3)

Question 13

Amount measured in

Answer 13

atoms
molecules
moles

Question 14

Temperature

Answer 14

Celcius (C)
Kelvin (K)

Question 15

Energy is measured in

Answer 15

Joule (J)
calorie (cal)

Question 16

Pressure

Answer 16

Pascal (Pa)
millimeters mercury (mm Hg)
atmosphere (atm)
torr, bar, psi

Question 17

kilo (k)

Answer 17

1,000

Question 18

centi (c)

Answer 18

0.01

Question 19

mili (m)

Answer 19

0.001

Question 20

micro (u)

Answer 20

0.000001 (5 zeros)

Question 21

nano (n)

Answer 21

0.000000001 (8 zeros)

Question 22

1 Kilometer =

Answer 22

1000 meters (1km = 1000m)

Question 23

1 centimeter =

Answer 23

0.01 meters (1cm = 0.01 m)

Question 24

1 millimeter =

Answer 24

0.001 meters (1mm = 0.001 m)

Question 25

1 micro meter =

Answer 25

0.000001 meters (1um = 0.000001 m)

Question 26

1 nano meter =

Answer 26

0.000000001 meters (1nm = 0.000000001 m)

Question 27

Density =

Answer 27

mass/volume

Question 28

cathode Ray Tibe Experiment

Answer 28

high voltage creates a stream of particles, they bent away from the negatively charged plate and towards the positively charged plate.
conclusion: existence of negatively charged particles (electrons)

Question 29

Rutherords Gold Foil Experiment

Answer 29

fired particles at sheet of gold foil, some passed through others bounced back.
conclusion: the mass of the atom is concentrated in the positive nucleus around which electrons move

Question 30

Discovery of neutron

Answer 30

James Chadwick

Question 31

Isotopes

Answer 31

same element, different number of neutrons, isotopes can be identified by their mass

Question 32

Mass Defect

Answer 32

amount of matter converted to energy when the nucleus of an atom is formed from protons + neutrons

Question 33

wavelength (lamda- upside down y)

Answer 33

distance between identical points in a wave

Question 34

frequency (v)

Answer 34

the number of peaks that pass through a point per unit of time

Question 35

Constructive Interference

Answer 35

“in phase” waves come together to become a bigger wave

Question 36

Destructive Interference

Answer 36

“out of phase” waves come together to cancel each other out

Question 37

Plum pudding model

Answer 37

neutrons + protons –> the dough
electrons –> plum bits scattered throughout

Question 38

Photoelectric effect + equation used

Answer 38

shinning light on a metal surface can cause e- to be ejected –> emitted e- are called photoelectrons
can measure photoelectron speed to determine their kinetic energy using =
KE electron = 1/2 (mass or electron)(velocity of electron)^2

Question 39

Light behaves as…

Answer 39

A wave and has particle like characteristics

Question 40

the minimum amount of energy required to detach an e- from a surface

Answer 40

KE electron = E photon - E0
0 = depends on metals identity

Question 41

Bohr Model

Answer 41

only works for H- atom (simplest) not 100% correct, electrons do not orbit nucleus on set tracks

Question 42

Heisenberg Uncertainty Principle

Answer 42

we cannot know both the position and speed of a particle, such as a photon or electron, with perfect accuracy; the more we nail down the particle’s position, the less we know about its speed and vice

Question 43

Schrodinger

Answer 43

propose mechanical model
–> treats electrons as waves, e- behaves as waves each having a wave function

Question 44

Schrodinger Equation

Answer 44

solution to the Schrodinger equation describes the 3D orbital shapes

Question 45

Probability Density function

Answer 45

determine the probability of finding the e- in a given region around the nucleus
square of the wave function gives us probability of density

Question 46

atomic orbital

Answer 46

region around the nucleus where the e- has 99% probability of being found

Question 47

s orbital

Answer 47

3D spherical shape

Question 48

p orbital

Answer 48

dumbbell shape

Question 49

d orbital

Answer 49

cloverleaf shape

Question 50

Pauli Exclusion Pirinciple

Answer 50

no two e- within an atom have the same set of four quantum numbers