2013 mrs redican – Flashcards

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What cannot be broken down or decomposed?
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elements
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What can be decomposed?
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compounds
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SOLIDS
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rigid, geometric, network lattice
definite shape and definite volume
particles vibrate in fixed position
closely packed particles
strong intermolecular forces
small distance between particles
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LIQUIDS
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definite volume , no definite shape
has surface tension and viscosity
particles can flow past one another
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GASES
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spreads to fill the entire container
no definite shape no definite volume
random, constant , straight-line motion
weak intermolecular forces
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INTERMOLECULAR FORCES
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forces between molecules
solids have strong forces, and gases have weak forces
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what is AVERAGE KINETIC ENERGY?
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energy of particle motion
TEMPERATURE
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when does potential energy change?
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changes during a phase change
energy of how the particles are spread out
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what are SUBSTANCES?
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elements and compounds
only one type of particle
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MIXTURES
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a combinations of elements and/or compounds
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PRESSURE-VOLUME OF GASES
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[image]
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KINETIC MOLECULAR THEORY OF GASES
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* gases move in constant random straight line motion
* gases do not lose or gain energy when they collide -- they have elastic collisions
*gas particles have a volume that is insignificant compared to the volume of the total gas
* average kinetic energy is temperature
* gas particles have no significant forces between them
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IDEAL GASES
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high temperature -- move very fast
low pressure -- very far apart
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MELTING
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solid -liquid equilibrium

(s)-->(l)

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VOLUME -TEMPERATURE OF GASES
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[image]
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FREEZING
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solid-liquid equilibrium

(l)-->(s)

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BOILING /EVAPORATION

VAPORIZATION

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liquid-gas equilibrium

(l)-->(g)

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CONDENSATION
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liquid-gas equilibrium

(g) --> (l)

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SUBLIMATION
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(s) --> (g)

like dry ice 

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DEPOSITION
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(g) --> (s)

like frost on your windows

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PHASE CHANGES
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temperature does NOT change

kinetic energy does not change

potential energy changes

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TEMPERATURE CHANGES
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kinetic energy changes
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1 MOLE
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6 x 10^23 particles
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MOLAR MASS
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gram formula mass
(add up the pieces using mass from the Periodic Table)
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SYNTHESIS
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A3 + 2B --> AB2
coming together to make one product
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DECOMPOSITION
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1 reactant breaking down into more than one product
AB ---> A + B
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SINGLE REPLACEMENT
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1 element and 1 compound replacing part of each other

A + BC --> B + AC
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DOUBLE REPLACEMENT
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compound 1 + compound 2 replacing part of each other
ex. PbCl + K(NO3) --> KCl + Pb(NO3)
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COMBUSTION
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CH + O2 ---> CO2 + H20
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PHYSICAL CHANGES
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boiling, melting, freezing, condensation, evaporation, solidifcation,sublimation, deposition
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5 types of CHEMICAL REACTIONS
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synthesis, decomposition, single replacement, double replacement, combustion
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ATOM
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the simplest unit of an element
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Which subatomic particles have mass?
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protons and neutrons
a mass of 1 amu each
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Which subatomic particle has almost no mass and is very small?
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electrons
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According to the wave mechanical model of the atom, where are electrons located?
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orbitals , regions of high probability of finding an e-
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VALENCE ELECTRONS
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electrons in the outermost shell (the last number in the e- configuration)
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ISOTOPES
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same protons and atomic number and symbol
different mass number and different numbers of NEUTRONS
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How do we calculate atomic mass?
( THIS IS NOT MASS NUMBER!!)
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mass multiply by abundance (in decimal percent , to the left, to the left like Beyonce :) The abundance decimal point gets moved NOT the mass.
C-12 mass 12.01 abundance 98.7%
(12x0.987) + ...
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ORBITALS
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the most likely region to find an electron
(areas of high probability)
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QUANTUM LEAP
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1) e- absorb energy
2) go to a higher level "excited state" (unstable)
3) go to a lower level
4) release a photon of light (bright line atomic spectra)
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MASS NUMBER
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number of protons + number of neutrons (added up)
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ATOMIC NUMBER
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number of protons
can be found on the periodic table
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ATOM ELECTRICALLY NETURAL
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because # of protons = # of electrons
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EXCITED STATE
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electron jumped up to a higher energy shell
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BRIGHT LINE ATOMIC SPECTRA
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unique "fingerprint" that can identify an element
produced when electron goes to a lower energy level and releases photon of light
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ALPHA
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positive and has the most mass
weakest power
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GAMMA
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most penetrating power
pure energy
no mass , no charge
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FISSION
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nuclear power
U + n --> Ba + Kr + 3 n + energy
to split apart
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FUSION
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H + H --> He + energy
to combine
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NATURAL TRANSMUTATION
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one element decaying and becoming a new element

X -->
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ARTIFICIAL TRANSMUTATION
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one element and a particle becoming a new element

X + beta/gamma/alpha --->
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USES OF RADIOISOTOPES
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I-131 thyroid treatment
Co-60 cancer
C-14 date organic material
U-238 date rocks
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PROS and CONS NUCLEAR POWER
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pros + cheap, clean, less pollution

cons - radioactive waste, possible breakdown and radiation leaks/sickness
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HALF_LIFE
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the time it takes for a sample size to decay with only half remaining
half-life is a steady, constant rate
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AVOGADRO'S LAW
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gases at the same temp and pressure, will have equal volume and equal number of molecules
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MOLAR RATIOS
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Given a balanced equation, if the problem goes from moles to moles - --use molar ratios to solve
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CONSERVATION OF MASS
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mass and charge are both conserved

Given a balanced equation
if a problem is about grams and grams - - use conservation of mass to add/subtract to find the answer
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VALENCE ELECTRONS
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electrons in the outermost shell
the last number in an electron configuration
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SIMILAR ELEMENTS
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have same number of valence e-
same group
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ACROSS A PERIOD
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radii get smaller (positive nucleus pulls e- inward)
IE increases
EN increases
less metallic character
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DOWN A GROUP
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atomic radii get larger, more e- shells
IE decreases
EN decreases
metallic character increases
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METALS
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lose e-
malleable
luster/shiny
solid (except mercury)
ductile
good conductors b/c of free mobile e- (sea of e-)
hi density
*they become totally different when they react to become ionic
want to lose e
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NONMETALS
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dull
brittle
solids or gases (except Br)
poor conductors (no free mobile e-)
want to gain e- , high EN
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IONIC BOND
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metals with nonmetals
transfer of e-
high melt point
dissolve /soluble in water
conducts in water (electrolyte)
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COVALENT BOND
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nonmetal with nonmetal
shares e-
low melt point
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POLAR covalent
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shares unevenly
EN difference high
asymmetrical
soluble in water
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NONPOLAR covalent
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shares evenly
EN difference low or zero
symmetrical
insoluble in water
poor conductor
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LEWIS DOT DIAGRAMS
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dot represent valence e-
if more than one atom present, show how the electrons are transferred (if ionic) or shared (if covalent)
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ENTHALPY
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heat energy
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ENDOTHERMIC
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heat is absorbed
A + heat --> B + C
feels cool , because the rxn absorbs energy from the surroundings
heat of reaction is +
Table I
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EXOTHERMIC
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heat is released
A --> B + C + heat
feels warm, because the rxn releases energy to the surroundings
heat of reaction is -
Table I
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ENTROPY
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disorder of a system
solid is least , gases are the most
the more molecules the more disorder
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Nature and SPONTANEOUS RXNS
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greater disorder , more entropy
usually also exothermic, but not always
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COLLISION THEORY
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there must be collisions for molecules to react
there must me sufficient energy to react
there must be more stability in the products formed
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REACTION RATE
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if the reaction rate increases, the time it takes is less
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TEMPERATURE AND RXN RATE
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higher temp, more kinetic energy, more collisions, faster rxn
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CONCENTRATION AND RXN RATE
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more particles per volume, more collisions, faster rxn
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SURFACE AREA AND RXN RATE
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crushing/powder, grinding makes more surface area for more possible collisions, faster rxn
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REACTIVITY OF ELEMENTS
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Table J, higher is more reactive
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CATALYST
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creates an alternate pathway with a lower activation energy ( faster)
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HEAT OF REACTION
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H products - H reactants
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ACTIVATION ENERGY
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the minimum energy required for the rxn to occur
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ACID
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H+ donor
H..., usually
sour
reacts with metals
pH below 7
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BASE
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H+ acceptor
...OH, usually
bitter
slippery
pH above 7
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NEUTRALIZATION
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Acid + Base ---> ionic salt and HOH
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MOLARITY
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moles of solute / liter of solution
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pH
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goes by factors of 10
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pH goes from 6 to 4
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increase H+ by 10*10 = 100 times more acidic
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pH goes from 11 to 8
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decrease in H+ 10^3 = 1000 less basic (going closer to neutral)
1/1000 of H+
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LEO
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lose electrons oxidation
oxidation # goes up
e- are on the product side
oxidized
reducing agent
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GER
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gain e- reduction
e- are on the reactant side
oxidation # goes down
reduced
oxidizing agent
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flow of e-
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always anode to cathode
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AN OX RED CAT
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anode is where oxidation occurs
cathode is where reduction occurs
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voltaic cell vs electrolytic
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voltaic requires a salt bridge that lets ions flow
voltaic, no battery , so it is spontaneous
voltaic : chemical energy converted to electrical

electrolytic requires a battery, not spontaneous
electrolytic : electrical energy converts to chemical energy
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solute vs solvent
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solute gets dissolved
solvent does the dissolving
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HETEROGENEOUS MIXTURES
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different particles not evenly spread out
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HOMOGENEOUS MIXTURES
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Solutions
if in water, aqueous
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SEPARATE BY SIZE
LIKE HETEROGENEOUS MIXTURES
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filtration (like sand and water)
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SEPARATE INKS DYES, COLORS
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chromatography
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SEPARATE BY BOILING POINT
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distillation
like crude oil (fractional distillation)
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SEPARATE BY EVAPORATION
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dissolved solids in water/liquids

like salt water
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ADDING MORE PARTICLES MAKE THE
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freezing point go down
boiling point go up
vapor pressure go down
osmotic pressure go up
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SUPERSATURATED, SATURATED, UNSATURATED
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supersaturated= above the accepted value,
saturated = equal to the accepted value
unsaturated = less than the accepted value
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PRECIPITATE
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Solid in solution,
occurs when something is insoluble
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What has a fixed ratio or proportion?
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compounds
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If a substance has a high boiling point what kind of intermolecular forces does it have?
Conversely, low boiling point?
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strong or high

Low boiling point means lower intermolecular forces
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Which two subatomic particles have the same quantity of charge but opposite signs?
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proton +1, and electron -1
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Which subatomic particle holds the nucleus together?
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neutrons
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Which subatomic particle is equal to the atomic number?
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protons only
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Which two subatomic particles have the same quantity of charge but opposite signs?
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proton +1, and electron -1
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Which subatomic particle holds the nucleus together?
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neutrons
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Which subatomic particle is equal to the atomic number?
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protons only
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Which subatomic particle has no charge?
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neutron
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Which subatomic particle has a charge of -1?
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electron
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What does NOT change during excited state?
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nucleus
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How do we calculate atomic mass of isotopes?
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take the weighted average of all the naturally occurring isotopes
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Mass into lots of energy
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nuclear power
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chemical energy into electrical
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voltaic cell
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electrical energy into chemical energy
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electrolytic cell
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How do the boiling points of water and a solution compare?
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the solution will have a higher boiling point and lower freezing point
(boiling pt elevation and freezing pt depression)
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How are C graphite and C diamond different?
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different structures so different properties
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How are allotropes different?
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different structures and different properties
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What makes something organic?
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Carbon
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What elements are in a hydrocarbon?
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H and C only
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What is a saturated molecule?
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all single bonds = alkanes
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What is an unsaturated molecule?
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contains at least 1 multiple bond (double or triple)
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-COO-
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ketone
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-COOH
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organic acid
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What reaction produces polymers?
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polymerization
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What reaction produces esters?
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esterification
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What reaction produces alcohol?
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fermentation
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CH4 + Cl2 ==> CH3Cl + HCl
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substitution
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What are esters made from?
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alcohol + organic acid
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What element can make long chains, rings and networks?
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carbon
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How many electrons are shared in a triple bond?
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6 e- or 3 pairs of e-
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What is equilibrium?
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when forward and reverse reaction rates are equal and the concentration of the reactants and the products remains constant
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What is Le Chatelier's Principle?
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that a system in equilibrium , when disturbed, will shift and return to equilibrium
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What type of bonding gives water an unusually high boiling point?
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hydrogen bonding
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What are the 3 types of hydrogen bonds?
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H-N H-O H-F
because of high EN
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A system in equilibrium, when pressure is increased will shift towards ________
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the side with less moles of gas
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A system in equilibrium, when pressure is decreased will shift towards ________
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the side with more moles of gas
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