chem final

energy

ability to do work

system

portion of universe of sample that is being studied

surroundings

remainder of universe

specific heat

amt of heat necessary to raise 1g of a substance to 1C

\

joule

SI unit for energy

calorie

amt of heat necessary to raise 1g of H2O to 1C

exothermic process

1. releases heat/gives heat to surroundings

2. ΔH (change in enthalpy) is negative,

3. products have lower energy than reactants

endothermic

1. reactions that absorb heat from surroundings

2. products have greater energy than reactants

3. ΔH is positive

first law of thermodynamics

energy cannot be created nor destroyed

entropy

ΔS, amount of disorder in a system

second law of thermodynamics

the entropty in the universe if increased of stays the same (drawn towards more disorder)

what does ΔH mean

change in enthalpy

what does ΔS mean

change in entropy

is this exo/endo?: ΔH is positive

endo

is this exo/endo?: products are lower than reactants

exo

is this exo/endo?: heat is given off to the surroundings

exo

is this exo/endo?: the reation feels cool to the touch

endo

ΔH f is

enthalpy of formation

the enthalpy of formation for any element in its standard state is ___ joules

0

when water turns to liquid to steam, entropy ___ __and ΔS is__ ____

idk why it did that but anyways the answers r INCREASE and POSITIVE

how are wavelength and frequency related to each other?

inversely

how are energy and frequency related to each other?

directly

what is the speed of light in a vacuum?

3\.0x10^8

what colors are of the visible spectrum in order from lowest to highest wavelength?

red orange yellow green blue indigo violet

which colors have the highest and lowest frequencies?

violet has highest frequency and shortest wavelength, red had lowest frequency and longest wavelength

light is both a…

wave and particle

pauli exclusion principle

no 2 electrons can have the same 4 quantum particles

aufbau principle

lower energy orbitals fill w/ electrons first

heisenburg uncertainty princple

it is impossible to know the position and momentum of any electron at the same time

line spectrum

specific wavelength given off by a particular element

ground state (of an electron)

lowest energy orbital an electron can occupy

excited state

when an electron occupies a higher orbital than the ground state

Orbital sublevel information

S - 1 orbital, 2 electrons per sublevel

P - 3 orbitals, 6 electrons per sublevel

D - 5 orbitals, 10 electrons per sublevel

F - 7 orbitals, 14 electrons per sublevel

how many electrons are on the third energy level of an atom

formula - 2n^2 → N = the energy level → 2(3)^2 = 18

what is the shape of an S orbital

a sphere

what is the shape of a P orbital

a dumbbell

metals

metallic, conduct electricity

non-metals

non metallic, do not conduct electricityh

halogens

group 17, highly reactive non metals

metalloids

on the stairstep, has properties of both metals and nonmetals

transition metals

groups 3-12

inner transition metals

lactinides and actinides (long 2 rows at the bottom of periodic table)

alkali metals

group 1, highly reactive metals that are soft

alkaline earth metals

group 2, less reactive than group 1

noble gases

group 18, stable/unreactive nonmetals

what is the most abundant element in the universe

hydrogen

what is the most electro negative element

Fluorine

how much of our air is made up of nitrogen

78%

how much of our air is mad eup of oxygen

21%

what is the only metal that turns to liquid at room temperature

mercury

what are the different forms of carbon?

black solid, coal, and diamond

are halogens easily attainable in their elemental form?

no

groups are … on the periodic table

columns

periods are …. on the periodic table

rows

are elements in the same group similar?

yes

does atomic radius increase of decrease if you go down a group on the periodic table?

increase

does AR decrease or increasde as you go from left to right on PT

decrease

ionization energy

minimum energy necessary to remove first electron from outermost energy level to form a cation

what is the trend for ionization energy down a group

decrease

what is the trend in electronegativity if you go from left to right

increase

what is the trend for electronegativity if you go down a group

decrease

why do elements bond

to achieve a lower energy lvl

wht is the octet rule

atoms will gain/lose/share an electron to achieve a noble gas configuration (8 valence electrons)

which element does not adhere to the octet rule

hydrogen

how do covalent bonds form

they share electrons

what elements make up covalent bonds

non-metal and non-metal

what are the main properties of covalent compounds

gases, liquids, low-melting solids, don’t conduct electricity

polar bond

unequal sharing of bonded electrons between 2 elements of different identities and electronegativities

non-polar bond

equal sharing of two elements that are of the same element

what do δ+ and δ− mean?

partial charge

which of the following bonds are polar: H-H, H-Cl, H-F

H-H

as the electronegativity difference increases between bonded atoms, what happens to the polarity of the bond

the polarity increases

how are ionic bonds formed

they transfer from metal to non-metal

what types of elements make up ionic bonds

metal and non-metal

what are the main properties of ionic compounds

solids, crystaline solids, high melting point, conducts electricity

what is electrostatic force

an attractive yet repulsive force caused by the electricity charges particles

how are metallic bonds formed

metals bond to metals

what is the theory that describes metallic bonds

sea of electrons theory

what are some of the properties for metallic bonds

shiny, conduct electricity, and malleable

what does a line mean in a lewis structure

a bond was formed

how many electrons are shared and a double and triple bond

4, and 6

what are lone pairs fo electrons

non-bonding electrons

solution

homogeneous mixture w/ 2 parts

solvent

substance in greater amounts and does the dissolving in the mixture

solute

substance in greater amounts that is in lesser amounts, that is getting dissolved in the mixture

miscible

mix completely to form one phase (example - hydrogen peroxide mixture)

immiscible

does not completely mix and forms 2 phases (oil and water)

dissociation

separation of an ionic substance into separate ions

the 3 ways to increase rate that sugar dissolves in water

mix, heat up, and crush

like dissolves like

general rule to solubility: polar dissolves polar and non-polar dissolves non-polar

saturated solution

dissolved as much solute in solvent that will stay in solution at equilibrium

unsaturated solution

solution that has less solute than it could at equilibrium

super saturated solution

solution that contains more solute than could stay in the solution at equilibrium

how does pressure affect the solubility of a gas in a liquid

increases solubility w/ increased pressure

how does temperature affect the solubility of a gas in a liquid

solubility of gas decreases w increasing temperature

molarity

M = mols of solute/liters of solution

molality

m = mols of solute/kg of solvent

colligative properties depend on … rather than the …

amount of particles, not the type

the boiling point of a liquid is where the …..

vapor pressure is the same as the atmospheric pressure

when solute is added to pure solvetn, what happens to the vapor pressure?

the vapor pressure increases