chem 1 exam Flashcards
Scientific Method
A through series of steps followed to solve problems including collecting data, forming a hypothesis, testing, and concluding.
Theory
A hypothesis that has been tested with a significant amount of data
Law
a descriptive statement or equation that reliably predicts events under certain conditions
Atom
smallest indivisible unit for an element
substance
a form of matter that has definite composition ad distinct properties
(CO2, NaCl)
Mixture
can be separated by physical means into its components without changing the identities of the components
molecule
consists of two or more atoms joined together by chemical bonds
Homogeneous mixture
uniform throughout
Heterogeneous mixture
not uniform
Solution
homogeneous mixture
physical property
can be observed and measured without changing the identity of the substance (boiling/melting point)
chemical property
one a substance exhibits as it interacts with another substance
Tera-
T, 10^12
Giga
G, 10^9
Mega
M, 10^6
Kilo
k
10^3
Deka
D
10^1
Hecto
H
10^2
Unit
1;base SI unit
Pico
10^-12
Deci
d
10^-1
Centi
c
10^-2
Nano-
10^-9
Micro
u
1x10^-6
Milli
10^-3
Atomic mass unit mass
1.66 x 10^-24 g
Atomic mass unit
used to express masses of atoms
C to K
K - 273.15
Liter
Volume
Fahrenheit to Celsius
F = (9/5) * C + 32
multiplying and dividing with SF
number with the smallest amount of sig figs in the og equations
1 kn to miles
1 km is .62 miles
1 lb to grams
454 grams
In to Cm
1 in = 2.54 cm
Addition/Subtraction with SF
the answer cannot have more digits to the right of the decimal point than any of the original numbers
Electron weight
9.10938 10^-28 g
Element
a substance that cannot be broken down into two or more simpler substances
Proton weight
1.67262 x 10^-24 g
Definite proportion
one chemical sample will be the same as another chemical sample
a chemical compound always contains the same elements in the same proportions by mass
Who discovered the Electron
Thomson
Neutron weight
SIMILAR TO PROTON
Proton Electron charge
Opposite of each other
Atomic number?
number of protons in the nucleus
Isotopes
have a different neutron number from their element
Mass number
the total number of protons and neutrons
Nucleons
protons + neutrons
Diatomic
contain two atoms and may be either hetero- or homo-
Ions
different charge from their element
Heteronuclear
different atoms
Super seven
Br, I, N, Cl, H, O, F
Alkali metals
1A
Homo nuclear
two atoms are the same
Alkaline earth metals
Group 2A
Mole mass
6.022 x 10^23
Chalcogens
Group 6A
Halogen
Group 7A
Noble gas
Group 8A, has all eight electrons
Transition metals
1B; 3B to 8B
Cations
postively charged ion
Anion
negatively charged ion
Mole defiintion
amount of substance that contains as many atoms as there are atoms in 12g of carbon 12
Who determined the charge to mass ratio of electrons?
Thomson
Solvent
liquid doing the dissolving
dilution
preparing a less concentrated solution from a more concentrated one
Who proposed the modern nuclear model?
Rutherford
Who proposed the plum pudding model?
Thomson
Who did the oil drop experiement
Milikan
WHo did the gold foil experiment
Rutherford
Who discovered the charge of the electron?
Milikan
Who discovered the law of definition proportions?
Dalton
Who dealt with cathode rays and electrons?
Thomson
Who formulated atomic theory
Dalton
1 calorie equals how many Joules?
4.184
How many cal in a Kcal or Calorie
1000
L = 0
s
L = 1
p
L= 2
d
L= 3
F
Kinetic energy
energy based on motion
potential energy
based on position
chemical, electrostatic
Joule
si unit of energy
Wavelength/Frequency proportion
Inverse
Constructive interference
adding in phase waves
Destructive inference
adding out of phase waves
Photons
particels of light
When is an electron excited the most
energy state in which n > 1
principal quantum number, n
describes size
angular moment quantum number, l
shape
magnetic quantum number
orentation, direction
Pauli exclusion principle
no two electrons in an atom can have the same four quantum numbers
Aufbau principle
states that electrons are added to the lowest energy orbitals first before moving to higher energy orbitals
Hund’s rule
the most stable arrangement of electrons is the one in which the number of electrons with the same spin is maximized
paramagnetic
one+ unpaired electrons
DIAMAGNETIC
all electrons paired
isoelectric
identical electron configurations to the noble gas to the right
atomic radius
distance between nucleus and outer shell
IE (ionization energy)
the minimun energy need to remove an electron from an atom in the gas phase
sheilding
an electron is partially shielded from the positive charge of the nucleus by the other electrons
electron
the energy released when an atom in the gas phase accepts an electron
