Mcat General Chemistry Lecture 1

Front 1

nuclide

Back 1

an atom of a specific isotope

Front 2

H-1

Back 2

protium

Front 3

H-2

Back 3

deuterium

Front 4

H-3

Back 4

tritium

Front 5

Avogadro's number

Back 5

the number of atoms in a mole, 6.02 x 10^23

Front 6

Phase of metals at room temperature

Back 6

solid

Front 7

Characteristics of alkali metals

Back 7

soft solids with low densities and low melting points

Front 8

Characteristics of alkaline earth metals

Back 8

Harder, more dense, melt at higher temperatures than alkali metals. Heavier alkaline earths more reactive than the lighter ones.

Front 9

Characteristics of 4A elements

Back 9

Form 4 covalent bonds. All but C forms 2 more bonds w/ Lewis bases.

Front 10

Characteristics of 5A elements

Back 10

Form 3 covalent bonds. All but N form 2 more bonds by using d orbitals. Lewis base can form 6th bond.

Front 11

atoms with ability to form pi bonds

Back 11

small atoms. B/c p orbitals overlap.

Front 12

chalogens

Back 12

6A elements

Front 13

atoms with ability to form more bonds

Back 13

large atoms. B/c of d orbitals.

Front 14

Characteristics of 7A

Back 14

more reactive at top of periodic table than at bottom.

Front 15

metalloids

Back 15

B to At (BAT), Ge and Sb

Front 16

ionization energy

Back 16

the energy needed to remove an electron from a nucleus.

Front 17

local maxima of ionization energy

Back 17

filled subshells, half filled p-subshells

Front 18

electron affinity

Back 18

the willingness of an atom to accept an additional electron. Peaks at halogens.

Front 19

electronegativity

Back 19

the tenancy of an atom to attract an electron in a ionic bond.

Front 20

w/ increasing atomic number, isoelectronic atoms...

Back 20

get smaller

Front 21

effective nuclear charge

Back 21

the amount of charge felt by an atom due to electron shielding. Greatest at right, bottom.

Front 22

mega

Back 22

10^6

Front 23

kilo

Back 23

10^3

Front 24

deci

Back 24

10^-1

Front 25

centi

Back 25

10^-2

Front 26

milli

Back 26

10^-3

Front 27

micro

Back 27

10^-6

Front 28

nano

Back 28

10^-9

Front 29

compound

Back 29

a substance made from two or more elements in definite proportions

Front 30

monatomic and simple polyatomic ions given the suffix...

Back 30

-ide

Front 31

polyatomic atoms w/ multiple oxygens given the suffix...

Back 31

-ite(less oxygenated) or -ate(more oxygenated)

Front 32

indicates fewest oxygens

Back 32

hypo-

Front 33

indicates most oxygens

Back 33

per-

Front 34

How is an acid named when the name of the anion ends in -ide.

Back 34

Acid begins in hydro- and ends in -ic.

Ex. Hydrosulfuric acid

Front 35

How are oxyacids named?

Back 35

Ending -ic used for species w/ more oxygens and -ous for species with fewer oxygens.

Ex. sulfuric acid (H2SO4) and sulfurous acid (H2SO3)

Front 36

metathesis

Back 36

a double displacement reaction

Front 37

Characteristics of crystalline solids

Back 37

sharp melting point and shape w/ well ordered structure of repeating units

Front 38

ionic crystals

Back 38

consist of oppositely charged ions held together by electrostatic forces.

Front 39

metallic crystals

Back 39

single metal atoms held together by delocalized electrons.

Front 40

network covalent crystals

Back 40

infinite network of atoms held together by polar and nonpolar bonds.

Front 41

molecular crystals

Back 41

individual molecules held together by intermolecular bonds.

Front 42

characteristics of an amorphous solid

Back 42

no characteristic shape. Melts over a temperature range.

Ex. glass.

Front 43

polymers

Back 43

solids with repeated structural units.

Front 44

rapid cooling of polymers results in...

Back 44

amorphous solid

Front 45

slow cooling of polymers results in...

Back 45

crystalline solid

Front 46

principle quantum number (n)

Back 46

designates shell.

Front 47

azimuthal quantum number (l)

Back 47

designates subshell (s, p, d, f). Determines shape.
l=n-1

Front 48

what numbers of l correspond to the s, p, d, and f subshells?

Back 48

l=0, s.
l=1, p.
l=2, d.
l=3, f.

Front 49

magnetic quantum number (ml)

Back 49

designates orbital of the subshell.
-l to +l.

Front 50

electron spin quantum number (ms)

Back 50

-1/2 or +1/2

Front 51

Pauli exclusion principle

Back 51

no two electrons in the same atom can have the same four quantum numbers.

Front 52

number of total orbitals w/in a shell equal to

Back 52

n^2

Front 53

Heisenberg uncertainty principle

Back 53

the more we know about the momentum of a particle, the less we can know about the position, and vice versa.

Front 54

aufbau principle

Back 54

with each new proton added to create a new element, a new electron is added as well.

Front 55

as electrons move further from the nucleus, energy level...

Back 55

rises

Front 56

Energy level rises as electrons move further from the nucleus b/c of...

Back 56

electrostatic potential energy from the separation of the electron from protons. Energy increases from a negative to zero as the electron moves an infinite distance from the nucleus.

Front 57

Ions are formed by...

Back 57

losing electrons from the orbital with the highest n value. If there are two orbitals w/ the same n value, they will be lost from the one w/ the highest l value.

Front 58

Hund's rule

Back 58

electrons will not fill any orbital in the same subshell until all orbitals in that subshell contain at least one electron. The unpaired electrons will have parallel spins.

Front 59

Planck's quantum theory

Back 59

electromagnetic energy is quantized. deltaE=hf, where h is planck's constant, 6.6x10^-34 and f is the frequency.

Front 60

Planck's constant (h)

Back 60

6.6 x 10^-34

Front 61

deBroglie's wavelength equation

Back 61

λ=h/mv or λ=h/p

Front 62

photoelectric effect

Back 62

electrons (photons) are emitted from matter as a consequence of their absorption of energy.