Lecture 1: Atoms, Molecules, and Quantum Mechanics

Question 1

the smallest piece of matter that still retains the qualities of that matter

Answer 1

element

Question 2

number of protons in the nucleus of an atom

Answer 2

atomic number (Z); written above elemental symbol in periodic table

Question 3

what defines an element?

Answer 3

number of proton in an element (atomic number); cannot have Carbon with 7 protons–this changes element to Nitrogen!

Question 4

negatively charged particle in an atom surrounding the nucleus; essentially massless; float / “orbit” around the nucleus

Answer 4

electron

Question 5

uncharged particle in the nucleus of the atom; can vary from versions of the same element to form elemental isotopes

Answer 5

neutron

Question 6

total number of protons and neutrons inside a nucleus

Answer 6

mass number (A)

Question 7

tiny particles of mass made of a nucleus made of protons and neutrons surrounded by electrons; means “uncuttable” but is really made of more fundamental particles

Answer 7

atom

Question 8

how many electrons can fill each orbital?

Answer 8

2 electrons

Question 9

things at a _____ Energy state get further from the body they are attracted to. This makes it easier to remove the item.

Answer 9

high; attractive force between two forces gets weaker

Question 10

quantum mechanics: electron energy shell; corresponds to row (period) in periodic table

Answer 10

n; elements in that period will have periods that fill the corresponding energy shell

Question 11

quantum mechanics: subshells

Answer 11

s, p, d, f

Question 12

electrons fill orbitals from _____ to _____ energy states

Answer 12

low to high energy states; electrons prefer their lowest energy state

Question 13

If an element is in groups 1 or 2, its highest E electron will be in the _____ subshell

Answer 13

S subshell

Question 14

If an element is in groups 13-18 (except He), its highest E electron will be in the _____ subshell

Answer 14

P subshell

Question 15

Equation: find # of moles in a sample

Answer 15

moles = grams / molar mass (g/mol)

Question 16

Equation: find # of grams from moles

Answer 16

grams = number of moles * molar mass (g/mol)

Question 17

SI unit: Mass

Answer 17

kilogram (Kg)

Question 18

Si unit: length

Answer 18

meter (m)

Question 19

SI unit: time

Answer 19

second (s)

Question 20

SI unit: electric current

Answer 20

Ampere (A)

Question 21

Si unit: temperature

Answer 21

Kelvin (K)

Question 22

SI Unit: luminous intensity

Answer 22

Candela (Cd)

Question 23

SI Unit: Amount of substance

Answer 23

Mole (mol)

Question 24

Mega (M)

Answer 24

10^6

Question 25

Kilo (k)

Answer 25

10^3

Question 26

Deci (d)

Answer 26

10^-1

Question 27

Centi (c)

Answer 27

10^-2

Question 28

Milli (m)

Answer 28

10^-3

Question 29

Micro (mu)

Answer 29

10^-6

Question 30

Nano (n)

Answer 30

10^-9

Question 31

Pico (p)

Answer 31

10^-12

Question 32

Femto (f)

Answer 32

10^-15

Question 33

Equation: Percent Comp

Answer 33

percent comp = molecular weight of element / molecular weight of entire molecule

Question 34

Find empirical formula of a compound from percent comp

Answer 34

1. Assume 100 g sample totranslate percent comp into grams 2. divide the # of grams of each substance by that element's molar mass to get number of MOLES of that element 3. Divide # of moles of each element by greatest common factor to get # of ATOMS rep/d by each element in emp form

Question 35

Equation: Percent Yield

Answer 35

Percent yield = (Actual yield / theoretical yield) * 100

Question 36

principal quantum number (n)

Answer 36

shell level corresponds roughly to the energy level of the elctrons within that shell larger n = greater size/energy of orbital

Question 37

azimuthal quantum number (l)

Answer 37

second quantum number subshell level describes shape of orbital (s, p, d, and f) value: from 0 to (n-1)

Question 38

magnetic quantum number (m1)

Answer 38

third quantum number designates precise orbital of each subshell value: between L and -L

Question 39

electron spin quantum number: m(s)

Answer 39

distinguishes between two electrons in the same orbital | values: -1/2 or +1/2

Question 40

Pauli exclusion principle

Answer 40

no two electrons in the same atom can have the same four quantum numbers. electrons in the same orbital must have opposite spins

Question 41

principle that arises from the dual nature of matter. there is inherent uncertainty in the product of hte position of a particle and its momentum the more we know about the momentum of any particple, the less we know about the position. Amount of uncertainty is on the order of Planck's constant

Answer 41

Heisenberg Uncertainty Principle

Question 42

Planck's constant (h)

Answer 42

6.63 * 10^-34 J*s

Question 43

Equation: Heisenberg Uncertainty Principle

Answer 43

h = ∆x * ∆p Note: h = Planck's constant ∆p = change in momentum

Question 44

demonstrates the electromagnetic energy is quantized (comes only in discrete units related to the wave frequency)

Answer 44

Planck's quantum theory

Question 45

Equation: change in energy by discrete increments

Answer 45

∆E = h * f | Note: h = Planck's constant

Question 46

Equation: Energy of a photon

Answer 46

E(photon) = h * f | Note: h = Planck's constant

Question 47

demonstrates a one-to-one photon to electron collision photon is released when electron falls to a lower energy shell electron is bumped up to its excited state after absorbing a photon

Answer 47

photoelectric effect

Question 48

Kinetic energy of electrons increases only when intensity in creased by increasing the _____ of each photon

Answer 48

frequency

Question 49

minimum amount of energy required to eject an electron from the surface of a metal

Answer 49

work function (theta)