Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
140 Cards in this Set
- Front
- Back
|
the study of structure and properties of matter
|
chemistry
|
|
|
one who studies the structure and properties of matter in order to figure out something or make something new
|
chemist
|
|
|
designs, builds, and operates a chemical plant
|
chemical engineer
|
|
|
an explanation of a phenomenon; must have a great deal of evidence
|
theory
|
|
|
a specific kind of matter
|
chemical
|
|
|
anything that has the property of inertia
|
matter
|
|
|
the tencency to maintain the present state of motion
|
inertia
|
|
|
the capacity to do work
|
energy
|
|
|
energy: motion, faster is more
|
kinetic energy
|
|
|
energy: position (where something could make it move); higher is more (in accordance to gravity)
|
potential energy
|
|
|
energy: transferred in electromagnetic waves
|
radiant energy
|
|
|
rule of nature
|
law
|
|
|
mass is conserved; mass can neither be created nor destroyed
|
law of conservation of mass
|
|
|
energy is conserved; energy can neither be created nor destroyed
|
law of conservation of energy
|
|
|
Einstein's revised law; mass-->energy, energy-->mass; the total amount of matter and energy in the universe is constant
|
law of conservation of mass/energy
|
|
|
observation --> problem
hypothesis --> educated guess experiment --> test analyze --> right or wrong |
scientific method
|
|
|
10^12 or 1,000,000,000,000
|
tera (T)
|
|
|
10^9 or 1,000,000,000
|
giga (G)
|
|
|
10^6 or 1,000,000
|
mega (M)
|
|
|
10^3 or 1,000
|
kilo (k)
|
|
|
10^-1 or 1/10
|
deci (d)
|
|
|
10^-2 or 1/100
|
centi (c)
|
|
|
10^-3 or 1/1000
|
milli (m)
|
|
|
10^-6 or 1/1,000,000
|
micro
|
|
|
10^-9 or 1/1,000,000,000
|
nano (n)
|
|
|
10^-12 or 1/1,000,000,000,000
|
pico (p)
|
|
|
converting units
e.g. convert 225 meters to megameters (225 m/1)(1 Mm/1,000,000)=.000225 Mm |
dimensional analysis
|
|
|
descriptive
|
qualitative
|
|
|
a number
|
quantitative
|
|
|
distance between two points; measured in meters (m); measured by meter stick
|
length
|
|
|
the amount of matter; measured in kilograms (kg); measured by balance scale
|
mass
|
|
|
interval between two events; measured in seconds (s); measured by a watch
|
time
|
|
|
averaged kinetic energy of particles; measured in kelvin (K); measured by thermometer
|
temperature
|
|
|
rate at which charge moves through a wire; measured in ampere (amp, A); measured by ammeter
|
electric current
|
|
|
measured in moles (mol)
|
chemical quantity of a substance
|
|
|
brightness; measured in candela (cd)
|
luminous intensity
|
|
|
amount of space; V=l*w*h; derived from length
|
amount of space
|
|
|
D=m/V; derived from mass and lenght
|
density
|
|
|
measure of force of gravity; SI unit is newton (N); 1 N=1kg*m/s^2; derived from mass, length, and time
|
weight
|
|
|
correctness
|
accuracy
|
|
|
reproducibility in a measurement
|
precision
|
|
|
general term meaning on e kind of matter
|
material
|
|
|
2 or more materials mixed together
|
mixture
|
|
|
physically separate part of a mixture
|
phase
|
|
|
the boundary between two phases
|
interface
|
|
|
mixture that is the same throughout e.g. salt water
|
homogeneous
|
|
|
mixture that is not the same throughout e.g. ice water
|
heterogeneous
|
|
|
a homogeneous mixture
|
solution
|
|
|
what is dissolved (the lesser amount) in a solution
|
solute
|
|
|
what the solute is dissolved in (greater amount)
|
solvent
|
|
|
a way to quantify the concentration of a solution
|
molarity
|
|
|
a homogeneous material that always has the same composition e.g. salt: NaCl, sulfur: S, water: H2O
|
substance
|
|
|
a substance made of only one kind of atom
|
element
|
|
|
a substance made of 2 or more kinds of atoms
|
compound
|
|
|
regardless of the amount of a compound it is always composed of the same elements in the same proportions
|
the law of definite proportions
|
|
|
when different compounds of the same elements are formed e.g. CO, CO2, CO3;always combine in small whole-number ratios
|
the law of multiple proportions
|
|
|
has a shape and volume; particles are close together
|
solid
|
|
|
has volume but no shape; particles aren't as close
|
liquid
|
|
|
has no shape or volume; particles are far apart
|
gas (vapor)
|
|
|
has no shape and no volume; particles very far apart
|
plasma (ionized gas)
|
|
|
removed electrons done by lots of heat; most matter in universe is on this state
|
ionized gas (plasma)
|
|
|
depends on the amount (mass, weight, volume)
|
extensive properties
|
|
|
not dependant on amount (color, shape, melting and boiling points, malleable, ductile, density)
|
intensive properties
|
|
|
change in a physical property; no new substance formed e.g. ice melts, still H2O
|
physical changes
|
|
|
attraction for molecules in paper
|
polarity
|
|
|
change in which new substance is formed; often energy is released or absorbed
|
chemical change
|
|
|
All matter is made of atoms.
All atoms of the same element are identical. Atoms combine in simple ratios to form compounds. |
John Dalton's Atomic Theory
|
|
|
number of protons in one atom of element (also number of electrons)
|
atomic number
|
|
|
an atom of the same element but with different mass because different number neutrons
|
isotope
|
|
|
one particular kind of atom
|
nuclide
|
|
|
a particle in the nucleus (proton, neutron)
|
nucleon
|
|
|
number of nucleons (protons + neutrons0
|
mass number
|
|
|
average mass of all the isotopes of an element (bottom number)
|
atomic mass
|
|
|
23
Na 11 How many protons? Neutrons? Electrons? |
11
12 11 |
|
|
characterized by lambda; measured in meters
|
wavelength
|
|
|
v=3.00*10^8
|
speed of light
|
|
|
developed quantum theory
|
Max Planck
|
|
|
radiant energy is not just waves it is also particles called photons or quanta (bundles of energy); energy of the light is not proportional the the intensity (brightness), it is related to frequency
Equation: E=hf, h=6.63E-34 electron gains energy and moves up to a higher energy level then drops back to its original energy level therefore gives off energy in the form of light |
Planck's quantum theory
|
|
|
the study of quanta or photons (very small particles)
|
quantum mechanics
|
|
|
developed the equation that relates particles to waves
|
Erwin Schrodinger
|
|
|
used Schrodinger's equation to calculate the probability of finding the electron in a hydrogen atom at any given position (53 picometers from nucleus)
|
Max Born
|
|
|
quantum number:
the energy level (principal quantum number); tells how many electrons are in each energy level (n=1 -> 2, n=2 -> 8, etc)...max #=2n^2; largest atoms have 7 energy levels |
n
|
|
|
quantum number:
the sublevel; s-->2 electrons, p-->6 electrons, d-->10 electrons, f-->14 electrons; n=1 --> s; n=2 --> s, p; n=3 --> s,p,d; n=4 --> s,p,d,f |
l
|
|
|
quantum number:
the orbital-path for 2 electrons; degenerate orbitals- orbitals that have the same amount of energy there same n and same l |
m
|
|
|
quantum number:
the spin of the electron (clockwise or counter clockwise); 2 electrons in the same orbital always have opposite spins |
s
|
|
|
no two electrons in the same atom have all four quantum numbers the same
|
Pauli Exclusion Principle
|
|
|
how difficult it is to stop a moving object; =mass*velocity; P=mv
|
momentum
|
|
|
It is impossible to know botht he position and the momentum of an electron simultaneously
|
Heisenberg Uncertainty Principle
|
|
|
model in which electrons spinning around the nucleus form a cloud of negative stuff
|
electron cloud model
|
|
|
arranged elements by atomic masses but found similar chemical properties where not just every 8; found pattern but there were some holes, turned out those elements had not been discovered yet
|
Dmitri Mendeleev
|
|
|
found very few exceptions to Mendeleev's pattern; arranged elements by atomic number then pattern worked
|
Henry Mosely
|
|
|
chemical properties of elements are a function of atomic numbers
|
periodic law
|
|
|
alkali metals
|
first group on periodic table
|
|
|
alkaline earth metals
|
second group on periodic table
|
|
|
chalcogens
|
sixteenth group on periodic table
|
|
|
halogens
|
seventeenth group on periodic table
|
|
|
noble gases
|
eighteenth group on periodic table
|
|
|
short columns on periodic table
|
transition elements (metals)
|
|
|
next to bottom row on periodic table
|
lanthanoids
|
|
|
bottom row on periodic table
|
actinoids
|
|
|
an atom with 8 electrons in its highest energy level is chemically stable
|
octet rule
|
|
|
electrons in the highest energy level
|
valence electrons
|
|
|
hard and shiny; solids; good conductors of heat and electricity; tend to have 1, 2, 3 valence electrons, malleable
|
metals
|
|
|
not hard or shiny; poor conductors; tend to have 5, 6, 7, 8, valence electrons; brittle (if solid)
|
nonmetals
|
|
|
have some properties of both metals and nonmetals
|
metalloids
|
|
|
radius of an atom; distance from nucleus to the highest electron; down a group - increases; across a period - decreases slightly
|
atomic radius
|
|
|
radius of an ion; if ion is positive by losing - decreases; if ion is negative gaining - decreases
|
ionic radius
|
|
|
energy required to remove the outermost electron; move across a period - increases (gets more difficult to remove); move done a group - decreases (shielding effect: how much stuff between nucleus and energy level)
|
first ionization energy
|
|
|
gain 1 electron, lose 1 electron, share its one elctron with another atom
|
ways hydrogen can bond with other elements
|
|
|
different structural forms of the same element
Carbon: 1. graphite: carbon in chains 2. diamond: carbon in diamond shape, much like baseball field Oxygen: 1. O2 in atmosphere 2. O3 ozone |
allotropes
|
|
|
one or more symbols sometimes with subscripts to represent a compound
|
chemical formula
|
|
|
electrostatic force holding ions together in an ionic compound; high melting points, soluble in water, good conductors of electricity in molten state, well defined crystals, large amount of energy released when formed
|
ionic bond
|
|
|
more than one atom becoming an ion
|
polyatomic ions
|
|
|
attraction of metal positive ions for the delocalized valence electrons
|
metallic bonding
|
|
|
mixture of a metal and another element
|
alloy
|
|
|
bond holding atoms together because they share electrons (to get 8 valence electrons); result is molecule; low melting point, poor conductor, brittle
|
covalent bond
|
|
|
molecules made of 2 atoms of the same element
|
diatomic molecule
|
|
|
which are diatomic molecules?
|
elements that end in "gen" or "ine"
|
|
|
name the prefixes in covalent compounds in order
|
mono
di tri tetra penta |
|
|
electronegativity difference is great
|
ionic
|
|
|
electronegativity difference is small
|
covalent
|
|
|
electronegativity of 1.67
|
either ionic or covalent
|
|
|
which type of bond, ionic or covalent, is most likely to be formed
|
bond character
|
|
|
the relative tendency to gain electrons when forming a bond
|
electronegativity
|
|
|
imaginary line in a molecule between the nucleus of one atom and the nucleus of another atom
|
bond axis
|
|
|
distance between the nucleus of one atom and the nucleus of another atom in a molecule
|
bond length
|
|
|
number of degrees between bond axes in a molecule
|
bond angle
|
|
|
radius of an atom not bonded to anything
|
atomic radius
|
|
|
raduis of an ion
|
ionic radius
|
|
|
radius of an atom that is covalently bonded to another atom
|
covalent radius
|
|
|
minimum distance between nucleus of bonded atom and next closes molecule
|
van der Waals
|
|
|
a compound that contains carbon; exceptions- CO2, CO;
|
organic compounds
|
|
|
name the organic prefixes in order
|
meth
eth prop but pent hex hept oct non dec |
|
|
two or more substance combined to form new substance
|
chemical reaction
|
|
|
AB+C --> CB+A
|
single displacement
|
|
|
AB+CD --> AD+CB
|
double displacement
|
|
|
A+B --> AB
|
synthesis
|
|
|
AB --> A+B
|
decomposition
|
|
|
organic compound + oxygen --> CO2 + H2O
|
combustion
|
|
|
Amadeo Avagadro
|
discovered number of particles
|
