Honots Chemistry 1 Semester 1 Review

smallest unit of matter

atom

element

pure substance

extensive properties

depends on size of the system

intensive properties

doesn't depend on the amount of matter present

physical change

doesn't change the identity of a substance

states of matter

solid, liquid, gas

chemical change

substance's ability to form a chemical reaction, changes the substance

homogeneous mixture

same throughout

heterogeneous mixture

mixture that is not the same throughout

mixture

material composed of two or more elements or compounds that are physically mixed together but not chemically combined

compound

more than one elemental symbol next to each other, pure substance

pure substance

element or compound that does not contain another element or compound

separation of mixtures

distillation, decanting, filtering, evaporation, chromatography

metal properties

good conductors of heat and electricity; malleable; solid at room temp; more dense than water; ductile; have luster

nonmetal properties

brittle, poor conductors of heat and electricity, gasses, liquids

metalloids properties

properties of both metals and nonmetals

periods

horizontal rows on the periodic table

groups

vertical columns on the periodic table

noble gas properties

least reactive, odorless, colorless

variables

factors that can change in an experiment

independent variable

causes dependent variable to change

dependent variable

changes in response to the independent variable

quantitative

data in the form of numbers

qualitative

data in the form of descriptions

observations

collecting data

scientific method

a logical approach to solving a problem

theory

hypothesis that can withstand multiple tests, can be revised

control

remains the same throughout an experiment

metric units volume

milliliters, cubic centimeters, liters

metric units temperature

kelvin, celsius

metric unit prefixed

tgmkhdbdcmunp

metric conversions

tgmkhdbdcmunp

density equation

d= m/v

density definition

ratio of mass to volume

weight

amount of gravitational pull on matter

metric unit mass

gram

precision

closeness among a group of data

accuracy

how close a measurement is to the true value

significant figures

all digits known with certainty plus an estimated digit

volume equation

V = m/d

number of electrons in an atom

atomic number

number of protons in an atom

atomic number

number of neutrons in an atom

mass number - atomic number

symbol of an isotope

\[element name] - mass number

law of multiple proportions

if two or more compounds are composed of the same two elements, then the ratio of the masses to the second element combined with a certain mass of the first element is always a whole number

law of multiple proportions scientist

dalton

gold foild experiment

alpha particles hit something small and dense where most of the mass was found; nucleus

gold foil experiment scientist

rutherford

dalton's atomic theory

all matter is composed of small particles called atoms, atoms of an element are identical in size, mass, and other properties, atoms can't be subdivided, created, or destroyed, atoms of different elements combine in simple whole number ratios to form compounds, in chemical reactions, atoms are combined, separated, and arranged

parts of dalton's atomic theory that were proven wrong

atoms of an element are identical in size mass and properties, atoms can't be subdivided

law of definite proportions

a single chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of sample or source of the compund

law of definite proportions scientist

proust

law of conservation of mass

mass is neither created nor destroyed during ordinary chemical reactions or physical changes

law of conservation of mass scientist

lavoisier

cathode ray tube

rays defected away negatively charged objects, electrons

cathode ray tube scientist

thomson

mole

unit of amount of substance

mole and mass

g/mol

molar mass

the mass in grams of one mole of a substance

moles to atoms equation

1 mol = 6.022 x 10^23 atoms

molar mass units

g/mol

converting mol to grams

grams x atomic mass

average atomic mass

the weighted average of the masses of all naturally occurring isotopes of an element

balance nuclear equation

you count protons and neutrons rather than counting atoms

positron

0/+1e, β

alpha particle

4/2 He

grams to mol

grams / molar mass

grams to atoms

divide by molar mass then multiply by 6.022 x 10^23

orbital notation

uses arrows pointing up or down to represent the electrons

principal quantum number

indicates the main energy level around the nucleus

angular momentum quantum number

tells the shape of an orbital

magnetic quantum number

indicates the orientation in space of an orbital

spin state quantum number

indicates the spin state of an electron

quantum numbers

principal, angular momentum, magnetic, spin

electron configuration rules

hund's rule, pauli exclusion principle, aufbau principle

hund's rule

each orbital must have one e- before pairing can occur

pauli exclusion principle

no two e- can have the same quantum numbers

aufbau principle

e- must occupy the lowest energy position

emission of a photon

electron falls to a lower energy level

line emission spectrum

e- absorb energy, e- move to a higher energy level, e- move back to ground state, e- release energy

frequency to wavelength equation

c=λv

frequency to energy equation

E=hv

photoelectric effect

electrons are emitted when light shines on a metal

ground state

the lowest allowable energy state of an atom

s sublevel shape

spherical

p sublevel shape

peanut/ dumbbell

d sublevel shape

double dumbbell

f sublevel shape

flower

energy levels

the possible energies that electrons in an atom can have

sublevels

s, p, d, f

highest occupied level in an atom

valence e-

electron configuration

the arrangement of electrons in an atom

noble gas notation

a way of writing the electron configuration of an atom that uses a nearby, prior noble gas (with a full octet) as a starting point

inner shell e-

two e-

frequency of electromagnetic spectrum

increases along the spectrum

wavelength

the distance between two corresponding parts of a wave

Dual nature of electromagnetic radiation

electromagnetic waves act as both a wave and a particle

number of orbitals in an energy level

increases throughout each sublevel

orientation of orbitals

magnetic quantum number

mendeleev's periodic table

arranged by atomic mass