Chemistry, Biology, Earth Science

Dissolves when added to a solution

unsaturated

Element subject to laboratory testing

Boyle

Synthetic element 111

roentgenium

Not three most common elements in the Earth's crust

magnesium

Magnesium is an

alkaline earth metal

Greatest ionization energy

Fluorine

Like fluorine in its chemical properties

chlorine

Halogen compound example

AlCl3

Forces for chemical bonding

Electromagnetic

Remains unchanged in reaction

mass

Number of atoms in (NH4)3PO4

20

Number of grams of B

6

CO and CO2 relationship

The mass ratio of oxygen to carbon is equal to the atom ratio in both compounds

Ion of sulfur charge

2-

Group 2A and Group 7A formula

MX2

Iron(III) bromide formula

FeBr3

Covalent compound example

NO2

Highest electronegativity value

Fluorine

Hydrogen bonding example

HF

Iron rusts is a

chemical change

3 Al2O3 contains how many Al atoms

6

Catalyst function

lowers the activation energy to start the reaction

Combustion reaction products

CO2 and H2O

Base dissolved in water property

react with active metals to liberate hydrogen

Anhydrous product of combustion

Water

Ten times as acidic as one of pH 4

3

Zn is where relative to Au in activity series

Above

One mole of hydrogen peroxide (molecules)

6.02x10^23

One mole of hydrogen peroxide (grams)

34.0

Covalent bonds oxygen forms

2

Bond angles in tetrahedron

109 degrees

Most common aromatic compound

benzene

Propane carbon atoms

three

C6H12 is named

hexene

Alkyl halide example

CH3Br

Ester general formula

R-COOR'

Unsaturated into saturated process

hydrogenation

Best-known synthetic polymer

plastics

Thomson discovery

the charge-to-mass ratio was the same for all materials

Nucleus discovery evidence

some radioactive particles were deflected by metal foil

Millikan experiment showed

the same or multiples of the same charge

Radius of an atomic nucleus determined by

measurements of radioactive particle deflections from gold foil

Neutral atoms have equal

all (atomic number number of electrons number of protons)

Solar system model problem

the electrons should lose energy since they are accelerating

Standard for masses of all other isotopes

carbon-12

Bohr theory explains

the colors in the hydrogen line spectrum

Narrow lines of colors in spectrum

line spectrum

Quantum mechanics theory is based on

the wave nature of electrons

Excited state to ground state transition

emits a photon

Moving particle has a wavelength concept

matter waves

Electrons arrangement in orbitals

electron configuration

Group IIA name

alkaline earth metals

A groups are called

representative elements

Chlorine belongs to

Halogens

Gain or loss of electrons forms

ion

Transition elements properties

all (metals B group variable charges)

Energy of a photon relationship

directly proportional to the frequency

Most energy color

Blue light

Lines of color pattern

are always the same with a regular spacing pattern

Hydrogen spectrum has

four color lines

Bohr model electron movement

jumping from one allowed orbit to another

Orbit farther from the nucleus to an orbit closer to the nucleus transition

emits a single photon with energy equal to the energy difference of the two orbits

Bohr model limitations

all (color lines in the hydrogen spectrum; could not explain the line spectrum of atoms larger than hydrogen; had some made-up rules without explanations)

Quantum numbers count

Four

Second main energy level and second sublevel notation

2p

Space where electron is found

orbital

Two different isotopes have

the same number of protons and electrons but different numbers of neutrons

Isotopes have

different masses and the same chemical behavior

Number of neutrons calculation

subtract the atomic number from the mass number

Mass number of an isotope is

always a whole number

Quantum mechanics and Bohr models explain

how electrons are able to emit light

Hydrogen line spectrum visible colors count

four

Photon is emitted when electron

jumps from a higher to a lower energy level

Hydrogen isotopes include

all (H-1 H-2 H-3)

Difference between C-12 and C-14

Number of neutrons

C-12 composition

6 protons 6 electrons and 6 neutrons

Not compound definition

a substance that cannot be broken down into simpler units

Smallest unit of an element

atom

Smallest particle of a compound

molecule

Chemical properties determined by

valence electrons

Outer orbital with eight electrons goal

octet rule

Family or group number indicates

total number of valence electrons

Magnesium ion symbol

Mg2+

Sharing electrons bond type

covalent bonds

Positive and negative ions bond type

ionic bond

Energy released of an ionic bond formation

heat of formation

Attract bonding electrons ability

electronegativity

Unequal sharing of electrons bond type

polar covalent

Chemical energy is

change of internal potential energy during a chemical reaction

Metallic bond property except

it restricts movement of electrons

Chemical reaction definition

chemical bonds are formed or broken

Energy released in photosynthesis

the same as the solar energy absorbed

Electrons in chemical bonding involve

valence electrons

Representative elements seek stability by

filling or emptying their outer orbitals

Ion formation purpose

loses or gains electrons to satisfy the octet rule

Family VIA charge

-2

Transfer of electrons bond type

Ionic

Sharing of two electrons bond type

Covalent

Salts are

Ionic compounds

Two bromide ions for each barium ion formula

BaBr2