Chemistry Exam 2

Front 1

Groups are located in what columns?

Back 1

Vertical columns.

Front 2

Periods are located in what columns?

Back 2

Horizontal columns.

Front 3

elements in group 1A are known as the what?

Back 3

Alkali Metals

Front 4

Elements in group 2A are known as the what?

Back 4

Alkaline earth metals

Front 5

Elements in group 7A are known as the what?

Back 5

Halogens

Front 6

Elements in group 8A are known as the what?

Back 6

Noble gases

Front 7

The elements found in the zigzag line are known as what?

Back 7

metalloids

Front 8

The block of elements in the center of the periodic table are known as?

Back 8

Transition elements

Front 9

The elements found in the first two columns to the left and the last six columns to the right are known as the what?

Back 9

representative elements

Front 10

Electrons have what type of charge?

Back 10

Negative

Front 11

Protons have what type of charge?

Back 11

Positive

Front 12

Neutrons have what type of charge?

Back 12

Neutral

Front 13

what subatomic particle's are found in the nucleus?

Back 13

Protons and neutrons

Front 14

What occupies the space surrounding the nucleus?

Back 14

Electrons

Front 15

the atomic number is the number of what?

Back 15

Protons in an atom

Front 16

The number above the elemental symbol is the what?

Back 16

Atomic number

Front 17

An atom is electrically.....positive, negative or neutral?

Back 17

Neutral

Front 18

The overall charge of an atom is what?

Back 18

Zero

Front 19

The mass number is the sum of what?

Back 19

protons and neutrons

Front 20

The number under the elemental symbol is the?

Back 20

Mass number

Front 21

Atoms of any one element can have a different number of what?

Back 21

Neutrons

Front 22

Atoms of the same element with different numbers of neutrons are known as what?

Back 22

Isotopes

Front 23

Why would we use an atomic symbol?

Back 23

To distinguish between the different isotopes of an element

Front 24

in an atomic symbol, where are the mass and atomic numbers located?

Back 24

Mass is in the upper left corner and atomic is in the lower left corner.

Front 25

Define atomic mass

Back 25

the weighted average of the masses of all of the naturally occurring isotopes of that element.

Front 26

What is the relative charge of a proton?

Back 26

+1

Front 27

What is the relative charge of a neutron?

Back 27

0

Front 28

What is the relative charge of an electron?

Back 28

-1

Front 29

Will the atomic number and mass numbers stay the same in an Isotope?

Back 29

The atomic number will, but the mass number will change

Front 30

The weighted average of the masses of all of the naturally occurring isotopes of an element is called the what?

Back 30

atomic mass

Front 31

What group of elements on the periodic table are not reactive and seldom found in combination with other elements?

Back 31

8A- the noble gases

Front 32

Soft shiny metals

Back 32

Alkali metals

Front 33

shiny, malleable, ductile and good conductor of heat and electricity

Back 33

metal

Front 34

elements with properties of both metals and nonmetals

Back 34

metalloid

Front 35

Shiny, poor conductor of heat and electricity

Back 35

nonmetal

Front 36

The maximum number of electrons allowed in any energy level is calculated using the formula..

Back 36

2n(2)

Front 37

A region in an atom where there is the highest probability of finding an electron is called an...

Back 37

Orbital

Front 38

a notation used to indicate the placement of the electrons of an atom in order of increasing energy.

Back 38

electron configuration

Front 39

The s block includes what groups?

Back 39

1A and 2A

Front 40

The p block includes what groups?

Back 40

groups 3A to Group 8A (not including the B's)

Front 41

Electrons in the outermost energy levels are known as...

Back 41

Valance electrons

Front 42

the distance from the nucleus to the energy level that contains the valence (outermost) electrons...

Back 42

atomic radius

Front 43

A diagram that shows the distribution of electrons in the orbitals of the energy levels is called an

Back 43

orbital diagram

Front 44

An orbital holds how many electrons?

Back 44

2

Front 45

What shape is the s orbital?

Back 45

spherical: Round

Front 46

S orbitals increase in size when?

Back 46

when the energy level n value increases

Front 47

P orbitals are found in what shape?

Back 47

figure 8

Front 48

In electron configuration abbreviations for what elements do we use He, Ne, or Ar?

Back 48

He= 3-10
Ne= 11-18
Ar= 19-36

Front 49

A negatively charged ion is called what?

Back 49

anion

Front 50

A positively charged ion is called what?

Back 50

Cation

Front 51

When atoms of one element combine with one or more atoms of a different element we call it what?

Back 51

A compound

Front 52

A sharing of valence electrons by atoms is what type of bond?

Back 52

Covalent bond

Front 53

A sharing of valence electrons by atoms is what type of bond?

Back 53

Covalent bond

Front 54

The group of symbols representing the elements in a compound with subscripts for the number of each is called a what?

Back 54

Formula

Front 55

an atom or group of atoms having an electrical charge because of a loss or gain of electrons is called what?

Back 55

an ion

Front 56

the attraction between oppositely charged ions is called what?

Back 56

ionic bond

Front 57

the difference between the number of protons and the number of electrons, written in the upper right corner of the symbol for the ion is called its what?

Back 57

ionic charge

Front 58

What is the octet rule?

Back 58

Representative elements react with other elements to produce a noble gas configuration with eight valence electrons.

Front 59

A group of covalently bonded atoms that has on overall electrical charge are called what?

Back 59

Polyatomic ions

Front 60

elements with 8 valence electrons are known as what?

Back 60

Octet

Front 61

In most covalent bonds who gains and who loses electrons?

Back 61

Metal loses and nonmetals gain