Studied by 0 peopleenergy
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
releases heat/gives heat to surroundings
ΔH (change in enthalpy) is negative,
products have lower energy than reactants
endothermic
reactions that absorb heat from surroundings
products have greater energy than reactants
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
Note
Flashcard