CHM1025 Exam 1

matter

anything that occupies space and has mass

energy

______ is not matter because it does not occupy space or have mass

pure substances and mixtures

matter can be broken up into what two groups

pure substances

type of matter with uniform composition throughout

elements and compounds

two types of pure substances

mixtures

two or more substances without uniform composition

elements

these cannot be broken down into smaller pieces

compounds

made up of one or more elements

heterogeneous and homogeneous

two different types of mixtures

solutions

homogeneous mixtures are also called _________

homogeneous

this type of mixture has a uniform composition

heterogeneous

this type of mixture does not have a uniform composition

homogeneous

sugar water is an example of a _________ mixture

heterogeneous

sand in water is an example of a _________ mixture

atoms

smallest unit of an element that maintains properties of that element

molecule

when two or more atoms come together, they form a ________

gas

physical state in which atoms are very loosely organized and moving quickly; always fit the container they're in; higher energy

liquid

physical state in which atoms are fairly unorganized; atoms flow around each other; fill as much of container as they can

solid

physical state in which atoms are rigidly positioned; don't care about shape of container; same volume

physical properties

things that can be measured without changing the object

physical properties

hardness, density, mass, volume, melting point are all examples of ________

mass

measure of how much matter is in an object (measured in grams)

volume

measure of how much space something occupies

density

ratio of an object's mass to volume

temperature

measure of how much heat an object has (celsius and kelvin)

0; 100

at what degree celsius does water freeze and boil?

0 K (-273.15 C)

what is the lowest possible temperature?

chemical properties

reactivity and chemical behavior of material

chemical changes

a change involving the breaking and forming of bonds between atoms

energy

capacity to do work or transfer heat

kinetic energy

energy of motion

potential energy

energy an object has based on position (often stored in bonds)

law of conservation of mass

no measurable change in mass occurs during a chemical reaction (1787)

law of definite proportions

all samples of the same compound always contain the same proportions by mass of the component elements (1797-1804)

all matter is composed of atoms, atoms of the same element are identical in mass and chemical properties/atoms of different elements have different masses and different chemical properties, atoms are not created or destroyed in chemical reactions, atoms combine in simple, fixed, whole number ratios to form compounds

points of daltons atomic theory

JJ thomson; cathode ray tube experiment

who discovered the electron and through what experiment

cathode ray tube experiment

experiment in which JJ Thomson noticed particles produced when an electric charge was applied to a CRT were attracted from a negative electrode to a positive electrode

RA Millikan's oil drop experiment

whose experiment determines electron's tiny mass

plum pudding model

thomson proposed which model of the atom

ernest rutherford

who conducted the gold foil experiment (1911)

gold foil experiment

experiment in which positively charged particles from radioactive source shot at a piece of gold foil; some particles went through, some deflected ; this experiment tells us there is dense region of positive charge

nucleus

rutherford proposed a _______, a small, dense, positively charged region at the center of an atom

james chadwick

__________ discovered the neutron (has mass but no charge)

atomic nuclear spin

james chadwick discovered the neutron while experimenting with _________, in which the mass of a proton and electron did not account for the atom's mass, and therefore the neutron is proposed

protons

atomic number is equal to the number of _________

isotopes

atoms of an element that contain the same number of neutrons

mass number

___________ is used to distinguish between isotopes

mass; atomic

in an isotope symbol, the _______ number is on top and the ________ number is on the bottom

ion

atomic species where number of protons does not equal number of electrons, and a charged particle forms

cation

a positively charged ion (# of protons>#of electrons)

anion

a negatively charged ion (#protons<#electrons)

atomic mass unit (amu)

1/12 the mass of a carbon-12 atom

relative atomic mass

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

relative atomic mass

isotope mass x present abundance

dimitri mendelev

in 1872, ____________ arranged the 60 known elements into groups by similar properties and ordered by atomic mass; space was left where trends suggested an element should exist but hasn't been discovered yet

across

rows/periods go ________ the periodic table

down

columns/groups go __________ the periodic table

alkali metals

group 1 in the periodic table

alkaline earth metals

group 2 in the periodic table

halogens

group 17 in the periodic table

noble gases

group 18 in the periodic table

hydrogen

which element is not considered an alkali metal, even though it's in group 1

transition metals

group 3-12 in the periodic table

lanthanides and actinides

at the bottom of the periodic table, the "f-block" consists of __________ and _________

metal

shiny solids with high melting points and are good conductors

nonmetal

not shiny, not malleable, not a conductor, low melting point

metaloid

exhibit properties of both metals and nonmetals

allotroph

one element that comes in multiple different forms

ionic compounds

contain oppositely charged ions in proportions to give electrical neutrality

ionic bond

has strong attractive forces in which electrons are transferred, not shared

molecular compound

composed of atoms from two or more nonmetals

covalent bond

discrete unit of atoms held together as a molecule

chemical formula

represents that lowest whole number ratio of atom/ions in a single formula unit of a compound

binary compounds

compounds containing atoms/ions of only two elements

monoatomic ions

ion of a single atom

Al3+, Zn2+, Ag+, Cd2+

exceptions to charges

oxoanions

many polyatomic ions bound to multiple oxygens

polyatomic ions

ions with more than one atom

electrolytes

ions that form on dissociation act as _______

strong

_________ electrolytes dissociate completely in water

NaCl

an example of a strong electrolyte

weak

__________ electrolytes only partially dissociated in water

sugar

an example of a weak electrolyte

molecular

__________ compounds are non or weak electrolytes

ionic

___________ compounds are typically strong electrolytes

acid

something that releases H+ in water

base

things that react with acids to produce water; produce OH- when added to water

first two rows of periodic table

what are the strong bases?

HI, HCl, HBr, HNO3, H2SO4, HClO4

6 strong acids

BO3^3-

borate

CO3^2-

carbonate

NO3^-

nitrate

NO2^-

nitrite

SiO4^4-

silicate

PO4^3-

phosphate

AsO4^3-

arsenate

AsO3^3-

arsenite

O2^2-

peroxide

SO4^2-

sulfate

SO3^2-

sulfite