chem final

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102 Terms

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energy
ability to do work
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system
portion of universe of sample that is being studied
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surroundings
remainder of universe
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specific heat
amt of heat necessary to raise 1g of a substance to 1C

\
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joule
SI unit for energy
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calorie
amt of heat necessary to raise 1g of H2O to 1C
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exothermic process

1. releases heat/gives heat to surroundings
2. ΔH (change in enthalpy) is negative,
3. products have lower energy than reactants
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endothermic

1. reactions that absorb heat from surroundings
2. products have greater energy than reactants
3. ΔH is positive
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first law of thermodynamics
energy cannot be created nor destroyed
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entropy
ΔS, amount of disorder in a system
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second law of thermodynamics
the entropty in the universe if increased of stays the same (drawn towards more disorder)
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what does ΔH mean
change in enthalpy
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what does ΔS mean
change in entropy
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is this exo/endo?: ΔH is positive
endo
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is this exo/endo?: products are lower than reactants
exo
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is this exo/endo?: heat is given off to the surroundings
exo
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is this exo/endo?: the reation feels cool to the touch
endo
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ΔH f is
enthalpy of formation
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the enthalpy of formation for any element in its standard state is ___ joules
0
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when water turns to liquid to steam, entropy ___ __and ΔS is__ ____
idk why it did that but anyways the answers r INCREASE and POSITIVE
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how are wavelength and frequency related to each other?
inversely
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how are energy and frequency related to each other?
directly
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what is the speed of light in a vacuum?
3\.0x10^8
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what colors are of the visible spectrum in order from lowest to highest wavelength?
red orange yellow green blue indigo violet
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which colors have the highest and lowest frequencies?
violet has highest frequency and shortest wavelength, red had lowest frequency and longest wavelength
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light is both a…
wave and particle
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pauli exclusion principle
no 2 electrons can have the same 4 quantum particles
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aufbau principle
lower energy orbitals fill w/ electrons first
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heisenburg uncertainty princple
it is impossible to know the position and momentum of any electron at the same time
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line spectrum
specific wavelength given off by a particular element
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ground state (of an electron)
lowest energy orbital an electron can occupy
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excited state
when an electron occupies a higher orbital than the ground state
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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
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how many electrons are on the third energy level of an atom
formula - 2n^2 → N = the energy level → 2(3)^2 = 18
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what is the shape of an S orbital
a sphere
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what is the shape of a P orbital
a dumbbell
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metals
metallic, conduct electricity
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non-metals
non metallic, do not conduct electricityh
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halogens
group 17, highly reactive non metals
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metalloids
on the stairstep, has properties of both metals and nonmetals
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transition metals
groups 3-12
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inner transition metals
lactinides and actinides (long 2 rows at the bottom of periodic table)
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alkali metals
group 1, highly reactive metals that are soft
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alkaline earth metals
group 2, less reactive than group 1
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noble gases
group 18, stable/unreactive nonmetals
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what is the most abundant element in the universe
hydrogen
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what is the most electro negative element
Fluorine
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how much of our air is made up of nitrogen
78%
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how much of our air is mad eup of oxygen
21%
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what is the only metal that turns to liquid at room temperature
mercury
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what are the different forms of carbon?
black solid, coal, and diamond
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are halogens easily attainable in their elemental form?
no
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groups are … on the periodic table
columns
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periods are …. on the periodic table
rows
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are elements in the same group similar?
yes
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does atomic radius increase of decrease if you go down a group on the periodic table?
increase
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does AR decrease or increasde as you go from left to right on PT
decrease
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ionization energy
minimum energy necessary to remove first electron from outermost energy level to form a cation
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what is the trend for ionization energy down a group
decrease
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what is the trend in electronegativity if you go from left to right
increase
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what is the trend for electronegativity if you go down a group
decrease
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why do elements bond
to achieve a lower energy lvl
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wht is the octet rule
atoms will gain/lose/share an electron to achieve a noble gas configuration (8 valence electrons)
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which element does not adhere to the octet rule
hydrogen
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how do covalent bonds form
they share electrons
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what elements make up covalent bonds
non-metal and non-metal
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what are the main properties of covalent compounds
gases, liquids, low-melting solids, don’t conduct electricity
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polar bond
unequal sharing of bonded electrons between 2 elements of different identities and electronegativities
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non-polar bond
equal sharing of two elements that are of the same element
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what do δ+ and δ− mean?
partial charge
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which of the following bonds are polar: H-H, H-Cl, H-F
H-H
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as the electronegativity difference increases between bonded atoms, what happens to the polarity of the bond
the polarity increases
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how are ionic bonds formed
they transfer from metal to non-metal
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what types of elements make up ionic bonds
metal and non-metal
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what are the main properties of ionic compounds
solids, crystaline solids, high melting point, conducts electricity
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what is electrostatic force
an attractive yet repulsive force caused by the electricity charges particles
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how are metallic bonds formed
metals bond to metals
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what is the theory that describes metallic bonds
sea of electrons theory
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what are some of the properties for metallic bonds
shiny, conduct electricity, and malleable
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what does a line mean in a lewis structure
a bond was formed
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how many electrons are shared and a double and triple bond
4, and 6
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what are lone pairs fo electrons
non-bonding electrons
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solution
homogeneous mixture w/ 2 parts
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solvent
substance in greater amounts and does the dissolving in the mixture
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solute
substance in greater amounts that is in lesser amounts, that is getting dissolved in the mixture
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miscible
mix completely to form one phase (example - hydrogen peroxide mixture)
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immiscible
does not completely mix and forms 2 phases (oil and water)
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dissociation
separation of an ionic substance into separate ions
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the 3 ways to increase rate that sugar dissolves in water
mix, heat up, and crush
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like dissolves like
general rule to solubility: polar dissolves polar and non-polar dissolves non-polar
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saturated solution
dissolved as much solute in solvent that will stay in solution at equilibrium
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unsaturated solution
solution that has less solute than it could at equilibrium
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super saturated solution
solution that contains more solute than could stay in the solution at equilibrium
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how does pressure affect the solubility of a gas in a liquid
increases solubility w/ increased pressure
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how does temperature affect the solubility of a gas in a liquid
solubility of gas decreases w increasing temperature
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molarity
M = mols of solute/liters of solution
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molality
m = mols of solute/kg of solvent
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colligative properties depend on … rather than the …
amount of particles, not the type
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the boiling point of a liquid is where the …..
vapor pressure is the same as the atmospheric pressure
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when solute is added to pure solvetn, what happens to the vapor pressure?
the vapor pressure increases