Mcat Chemistry Lecture 1

Front 1

All mass consists of ____

Back 1

atoms

Front 2

Atoms consist of ____

Back 2

protons, neutrons and electrons.

Front 3

Protons and neutrons collectively are ____ and held together by ____.

Back 3

nucleons
strong nuclear force

Front 4

Neutron is ____.
Charge on proton is ____.
Charge on electron is ____.

Back 4

neutral
positive
negative

Front 5

Charge on electron is ____.

Back 5

1 electron unit =
1.6 x 10^-19 coulombs.

Front 6

Most of an atom is ____.

Back 6

space.

Front 7

Atom has same number of protons and electrons unless it is an ___, in which case it has a different number of protons and electrons and thus carries a ____.

Back 7

ion
net charge

Front 8

Any single atom must be one of many ____.

Back 8

elements

Front 9

Element cannot be separated into smaller parts by ____ means

Back 9

chemical

Front 10

We represent an element by its ____

Back 10

chemical symbol.

Front 11

The ____ is the number of protons.

Back 11

atomic number

Front 12

The ____ is the identity of the element.

Back 12

atomic number

Front 13

The ____ is how many protons plus neutrons the atom has.

Back 13

mass number

Front 14

Isotopes have same number of ____ but different numbers of ____.

Back 14

protons
neutrons

Front 15

Carbons isotopes are particularly important because ____ is based on carbon 12.

Back 15

Avogadro's number

Front 16

The number of atoms in a 12g sample of carbon is Avogadro's number = ____

Back 16

6.02 x 10^23

Front 17

1 mole = ____

Back 17

6.022 x 10^23

Front 18

____/____ = amu

Back 18

grams/mole

Front 19

____ is weighted weight of all naturally occurring isotopes.

Back 19

atomic weight

Front 20

An ____ is about the mass of a proton or a neutron.

Back 20

amu

Front 21

The ____ is also defined by carbon 12, 1 atom of carbon 12 has a mass of ____ (si abbreviation of ____ is ____)

Back 21

amu
12 amu
amu
u

Front 22

Periodic table
row =
column =

Back 22

period
group or family

Front 23

Elements w/in a family are ____

Back 23

chemically similar

Front 24

First 2 families are the ____.

Back 24

alkali metals
alkaline earth metals

Front 25

The last 2 families are the ____.

Back 25

halogens
noble gases

Front 26

Periodic trends:

Back 26

Electro negativity
Electron affinity
Energy of ionization
Atomic radius
Metallic character

Front 27

If a trend starts with an e it increases to the ____.

Back 27

right and up a periodic table.

Front 28

The ____ is largest in the lower left hand corner.

Back 28

atomic radius

Front 29

The ____ increases as we move down and to the left on the periodic table.

Back 29

metallic character

Front 30

Metallic characteristics:

Back 30

thermal
electrical conductivity
ductility
malleability

Front 31

____ energy required to detach an electron from an atom

Back 31

Ionization energy

Front 32

Also becomes greater as you move more electrons, so the second is greater than the first, that is more energy is required to move the second electron than the first.

Back 32

Ionization energy

Front 33

____ - is the tendency of an atom to attract an electron that is in a bond shared by another atom

Back 33

Electro negativity

Front 34

____ - tells us how much an atom attracts electrons in a bond.

Back 34

Electron Negativity

Front 35

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

Back 35

Electron Affinity

Front 36

____ - tells us how much a lone atom attracts an electron.

Back 36

Electron Affinity

Front 37

____ is the sharing of a pair of electrons

Back 37

Covalent bond

Front 38

____ are distinct and separate repeating groups of 2 or more atoms held together by a covalent bond

Back 38

Molecules

Front 39

Nuclei ____ each other,

Back 39

repel

Front 40

The ____ is where the energy is the lowest.

Back 40

bond length

Front 41

Nature like the ____ possible, so will move the nuclei where the _____ is the ____.

Back 41

lowest energy
overall energy
lowest

Front 42

____ is energy from the reverse point of view, high ____ indicates a low energy molecule.

Back 42

Bond energy
bond energy

Front 43

To move the nuclei closer or farther apart requires ____, always require ____ to break a bond.

Back 43

energy
energy

Front 44

By bond energy we really mean bond ____, the bond energy is the amount of energy to ____ a bond.

Back 44

dissociation energy
break

Front 45

Energy is never ____ by breaking a bond, energy is released by bonds ____ in transition states.

Back 45

released
reformed

Front 46

A collection of atoms held together by bonds is a ____.

Back 46

compound

Front 47

A ____ is one of a group of distinct and separate repeating units, salt is a compound but not a ____ because the elements are not distinctly grouped.

Back 47

molecule
molecule

Front 48

The atomic composition of a compound can be described with an ____ that gives the ratio of the atoms.

Back 48

empirical formula

Front 49

CH2O is the _____ for glucose, also has a _____ C6H12O6, which gives the exact amount of atoms in the molecule.

Back 49

empirical formula
molecular formula

Front 50

Only ____ can have molecular formulas.

Back 50

molecular compounds

Front 51

Atomic weight of all the atoms of one element and divide it by all the atoms in the empirical formula =

Back 51

specific atom percent mass

Front 52

____ does not create new compounds like melting.

Back 52

Physical reaction

Front 53

____ does create new compounds, like combustion.

Back 53

Chemical reaction

Front 54

____ is the one that limits the reaction. The one that is used up first.

Back 54

Limiting reagent

Front 55

Reactions don’t always run to ____, it may reach ____ or may have ____ reactions.

Back 55

completion
equilibrium
competing

Front 56

____ = amount of product one would get if it ran to completion with no competing reactions.

Back 56

Theoretical Yield

Front 57

____ = Actual Yield / Theoretical Yield.

Back 57

Percent Yield

Front 58

Solids can by ____ or ____

Back 58

crystalline
amorphous

Front 59

_____ have a sharp melting point and a well ordered structure of repeating units.

Back 59

Crystalline solids

Front 60

Table salt and ice are ____ one with ions one with molecules.

Back 60

crystalline solids

Front 61

Crystalline solids are ____

Back 61

ionic
metallic
network covalent.

Front 62

____ - network covalent of carbon bonds.

Back 62

Diamond

Front 63

____ melts over a range and has no characteristic shape - glass.

Back 63

Amorphous solid

Front 64

____ - a special type of solid with repeating units, can be crystalline or amorphous, rapid cooling generally results in an amorphous solid and slow crystalline.

Back 64

Polymer

Front 65

DNA, glycogen and protein are all ____.

Back 65

polymers

Front 66

____ are like the address of the electron in a given atom.

Back 66

Quantum numbers

Front 67

Each electron has a set of ____, that tell us about the position and energy level of the electron.

Back 67

unique 4 quantum numbers

Front 68

The ____ tells us which shell the electron is in.

Back 68

principal quantum number

Front 69

The ____ are like energy levels, the further from the nucleus the ____.

Back 69

shells
more energy

Front 70

Each ____ represents a new principal quantum number .

Back 70

period

Front 71

____ = subshell, the possible values are from 0 to one less than the principal quantum number. They are described by S, P, D, F. S=0, P = 1 etc.

Back 71

Azimuthal quantum number

Front 72

____ = orbital in the subshell, the possible values are all integers from the negative value to the positive value of the azimuthal quantum number.

So from P subshell, could have 3 possible values -1, 0 and 1.

Back 72

Magnetic quantum number

Front 73

____ = distinguish between the two electrons in each orbital either positive 1/2 or negative 1/2.

Back 73

Spin number

Front 74

Pauli exclusion principal - ____

Back 74

no two electrons can have the same 4 quantum numbers.

Front 75

Heisenberg uncertainty principle - ____

Back 75

the more you know about position the less you know about momentum and vice versa

Front 76

____ - the orbital with the lowest energy will be contained in the subshell with the lowest energy, electrons will fill the orbital's with the lowest energy first

Back 76

Aufbau principle

Front 77

____ - some transition metals 4s and 3d, they are at the same energy level so certain cases electrons will add to empty 3d before 4s (just be aware it happens)

Back 77

Degenerate orbital's

Front 78

____ - electrons will add to empty orbital's at the same energy level before they fill any orbital at that level

Back 78

Hunds rule

Front 79

____ - electromagnetic energy is quantized, changes in discrete amounts, each discrete packet is a photon

Back 79

Planck's Quantum theory
E=HF,
E is energy, H is Planck's constant, F is the frequency of the light

Front 80

____ - light is made of particles called photons, elec

Back 80

Photoelectric effect

Front 81

Photons are released when an electron drops from a ____ energy level to a ____ energy level and a ____ can bump an electron to a higher energy level (farther from the nucleus).
The ____ must have a minimum amount of ____ to bump it up, if not it will just deflect.

Back 81

high
low
photon
photon
energy

Front 82

Light is made of individual pieces.

Back 82

photoelectric effect

Front 83

The photoelectric effect is seen by light is shown on a substance ant knocks off electrons, if the lights ____ is too low no photoelectric occurs, no matter how great the ____ of the light.

Turning up the ____ does not help because of the ____ characteristic of light. That is adding more ____ does not help.

Back 83

frequency
intensity
intensity
particle
photons

Front 84

Ions like to form a ____ configuration, cations always form from losing electrons from the ____.

Back 84

noble gas
highest energy subshell

Front 85

____ - electrons of the atom, count the electrons and list them in the order of their subshells from lowest to highest.

Back 85

Electron configuration

Front 86

Electron Config chart

Back 86

s p d f
1 s
2 s p
3 s p d
4 s p d f
5 s p d f