Chemestry Test Chapters 5,6,7

Front 1

The lowest allowable energy state of an atom is called its

Back 1

ground state

Front 2

Bohr's model of the atom predicted the

Back 2

frequencies

Front 3

THe smaller an electrons orbit the ______ the atoms energy level

Back 3

lower

Front 4

The larger an electron's orbit the ______ the atom's energy level

Back 4

higher

Front 5

When energy is added to a hydrogen atom it's _________ moves to a higher-energy orbit

Back 5

electron

Front 6

What is Heisenberg uncertainty principle?

Back 6

States that it is impossible to know both the velocity and position of a particle at the same time

Front 7

What is Schrodinger wave equation?

Back 7

It led to the quantum mechanical model of the atom.

Front 8

Each orbital may contain____electrons

Back 8

two

Front 9

All s orbitals are

Back 9

spherically shaped

Front 10

There are _____ equal energy p orbitals.

Back 10

3

Front 11

What is the electron configuration?

Back 11

The arrangement of electrons in an atom.

Front 12

THe arrangement of electrons is the most stable stable arrangement is called the atom's

Back 12

groundstate electron configuration

Front 13

THe Pauli exclusion principle states that

Back 13

a maximum of two electrons may occupy a single atomic orbital

Front 14

Hund's rule states

Back 14

that single electrons with the same spin must occupyeach equal energy orbital before additional electrons with opposite spins occupy the same orbital,

Front 15

What is the noble-gas notation

Back 15

Uses bracketed symbol nearest preceding noble gas atom in the periodic table.

Front 16

The electrons in the most outermost orbitals are called

Back 16

valance electrons

Front 17

What is the law of octaves?

Back 17

the properties of the elements repeated every eight elements.

Front 18

THe first periodic table was created by

Back 18

Dmitri Mendeleev

Front 19

In Mendeleev's periodic table elements were in order from

Back 19

increasing atomic mass

Front 20

Who arranged the periodic table a second time?

Back 20

Henery Mosley

Front 21

How did Mosley organize the periodic table?

Back 21

In increasing atomic number

Front 22

What is a column in the periodic table

Back 22

GROUP

Front 23

What is a row in the periodic table

Back 23

period

Front 24

Group A elements

Back 24

transition metals

Front 25

elements that conduct energy

Back 25

metals

Front 26

Group B elements

Back 26

transition metals

Front 27

THere are ___ main classifications of elements

Back 27

three

Front 28

Into many blocks is the periodic table divided?

Back 28

four

Front 29

How many d blocks are there?

Back 29

40

Front 30

What is ionization energy?

Back 30

the energy required to remove an electron from a gaseous atom.

Front 31

What does the electronegativity of an element indicate?

Back 31

indicates its atoms ability to attract electrons in a chemical bond.

Front 32

What do all elements in a group have in common?

Back 32

THe share the same # of valance elec.

Front 33

Alkali metals are

Back 33

shiny gray solids, soft enough to be cut with a knife

Front 34

Alakline earth metals form ions with a ____ charge

Back 34

2+

Front 35

The P-block contains

Back 35

metals, metalloids, nonmetals, noble gases

Front 36

___ is the most abundant element in the earths crust

Back 36

Aluminum

Front 37

Plants and animals get the nitrogen they need from

Back 37

nitrogen-fixing bacteria

Front 38

Ozone is

Back 38

an allotrope of oxygen

Front 39

How can a metal be a temparary magnet?

Back 39

When there is an unpaired electron in in the valance orbital of a metal atom or ion

Front 40

needed for the development of red blood cells

Back 40

cobalt

Front 41

The best conductor of electricity

Back 41

silver

Front 42

Atomic Radius is

Back 42

The size of the atom

Front 43

Atoms get ___ when moving down the periodic table

Back 43

bigger

Front 44

Atoms get ___ when moving across the periodic table

Back 44

smaller

Front 45

S orbial holds ____ pairs of electrons

Back 45

1

Front 46

P orbial holds ____ pairs of electrons

Back 46

3

Front 47

D orbial holds ____ pairs of electrons

Back 47

5

Front 48

F orbial holds ____ pairs of electrons

Back 48

7

Front 49

Alkaline earth metals

Back 49

somewhat soft,
less reactive than Alkali metals,

Front 50

Transition Metals

Back 50

Most gray, hard, and dense
less reactive than Alkaline earth metals

Front 51

Other Metals

Back 51

Softer than transition metals,
gray and malleble
less reactive than most metals

Front 52

Metaloids

Back 52

Properties between those of metals and Non-metals

Front 53

Halogens

Back 53

Very reactive
can form a compound with almost all metals
commonly used as cleaners

Front 54

Noble Gases

Back 54

colorless odorless gasses at room temp.
chemically inert

Front 55

other non-metals

Back 55

Life elements
light, non-metallic
poor conductors of heat and elec.

Front 56

Lanthanides and Actinides

Back 56

Rare earth metals
most reactive