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2013 mrs redican
elements, compounds,etc
141
Chemistry
11th Grade
10/16/2012

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

solid -liquid equilibrium

(s)-->(l)

Term
VOLUME -TEMPERATURE OF GASES
Definition
[image]
Term
FREEZING
Definition

solid-liquid equilibrium

(l)-->(s)

Term

BOILING /EVAPORATION

VAPORIZATION

Definition

liquid-gas equilibrium

(l)-->(g)

Term
CONDENSATION
Definition

liquid-gas equilibrium

(g) --> (l)

Term
SUBLIMATION
Definition

(s) --> (g)

like dry iceĀ 

Term
DEPOSITION
Definition

(g) --> (s)

like frost on your windows

Term
PHASE CHANGES
Definition

temperature does NOT change

kinetic energy does not change

potential energy changes

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

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

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

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

cons - radioactive waste, possible breakdown and radiation leaks/sickness
Term
HALF_LIFE
Definition
the time it takes for a sample size to decay with only half remaining
half-life is a steady, constant rate
Term
AVOGADRO'S LAW
Definition
gases at the same temp and pressure, will have equal volume and equal number of molecules
Term
MOLAR RATIOS
Definition
Given a balanced equation, if the problem goes from moles to moles - --use molar ratios to solve
Term
CONSERVATION OF MASS
Definition
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
Term
VALENCE ELECTRONS
Definition
electrons in the outermost shell
the last number in an electron configuration
Term
SIMILAR ELEMENTS
Definition
have same number of valence e-
same group
Term
ACROSS A PERIOD
Definition
radii get smaller (positive nucleus pulls e- inward)
IE increases
EN increases
less metallic character
Term
DOWN A GROUP
Definition
atomic radii get larger, more e- shells
IE decreases
EN decreases
metallic character increases
Term
METALS
Definition
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
Term
NONMETALS
Definition
dull
brittle
solids or gases (except Br)
poor conductors (no free mobile e-)
want to gain e- , high EN
Term
IONIC BOND
Definition
metals with nonmetals
transfer of e-
high melt point
dissolve /soluble in water
conducts in water (electrolyte)
Term
COVALENT BOND
Definition
nonmetal with nonmetal
shares e-
low melt point
Term
POLAR covalent
Definition
shares unevenly
EN difference high
asymmetrical
soluble in water
Term
NONPOLAR covalent
Definition
shares evenly
EN difference low or zero
symmetrical
insoluble in water
poor conductor
Term
LEWIS DOT DIAGRAMS
Definition
dot represent valence e-
if more than one atom present, show how the electrons are transferred (if ionic) or shared (if covalent)
Term
ENTHALPY
Definition
heat energy
Term
ENDOTHERMIC
Definition
heat is absorbed
A + heat --> B + C
feels cool , because the rxn absorbs energy from the surroundings
heat of reaction is +
Table I
Term
EXOTHERMIC
Definition
heat is released
A --> B + C + heat
feels warm, because the rxn releases energy to the surroundings
heat of reaction is -
Table I
Term
ENTROPY
Definition
disorder of a system
solid is least , gases are the most
the more molecules the more disorder
Term
Nature and SPONTANEOUS RXNS
Definition
greater disorder , more entropy
usually also exothermic, but not always
Term
COLLISION THEORY
Definition
there must be collisions for molecules to react
there must me sufficient energy to react
there must be more stability in the products formed
Term
REACTION RATE
Definition
if the reaction rate increases, the time it takes is less
Term
TEMPERATURE AND RXN RATE
Definition
higher temp, more kinetic energy, more collisions, faster rxn
Term
CONCENTRATION AND RXN RATE
Definition
more particles per volume, more collisions, faster rxn
Term
SURFACE AREA AND RXN RATE
Definition
crushing/powder, grinding makes more surface area for more possible collisions, faster rxn
Term
REACTIVITY OF ELEMENTS
Definition
Table J, higher is more reactive
Term
CATALYST
Definition
creates an alternate pathway with a lower activation energy ( faster)
Term
HEAT OF REACTION
Definition
H products - H reactants
Term
ACTIVATION ENERGY
Definition
the minimum energy required for the rxn to occur
Term
ACID
Definition
H+ donor
H..., usually
sour
reacts with metals
pH below 7
Term
BASE
Definition
H+ acceptor
...OH, usually
bitter
slippery
pH above 7
Term
NEUTRALIZATION
Definition
Acid + Base ---> ionic salt and HOH
Term
MOLARITY
Definition
moles of solute / liter of solution
Term
pH
Definition
goes by factors of 10
Term
pH goes from 6 to 4
Definition
increase H+ by 10*10 = 100 times more acidic
Term
pH goes from 11 to 8
Definition
decrease in H+ 10^3 = 1000 less basic (going closer to neutral)
1/1000 of H+
Term
LEO
Definition
lose electrons oxidation
oxidation # goes up
e- are on the product side
oxidized
reducing agent
Term
GER
Definition
gain e- reduction
e- are on the reactant side
oxidation # goes down
reduced
oxidizing agent
Term
flow of e-
Definition
always anode to cathode
Term
AN OX RED CAT
Definition
anode is where oxidation occurs
cathode is where reduction occurs
Term
voltaic cell vs electrolytic
Definition
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
Term
solute vs solvent
Definition
solute gets dissolved
solvent does the dissolving
Term
HETEROGENEOUS MIXTURES
Definition
different particles not evenly spread out
Term
HOMOGENEOUS MIXTURES
Definition
Solutions
if in water, aqueous
Term
SEPARATE BY SIZE
LIKE HETEROGENEOUS MIXTURES
Definition
filtration (like sand and water)
Term
SEPARATE INKS DYES, COLORS
Definition
chromatography
Term
SEPARATE BY BOILING POINT
Definition
distillation
like crude oil (fractional distillation)
Term
SEPARATE BY EVAPORATION
Definition
dissolved solids in water/liquids

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

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