chapter 1

Question 1

atomic # =

Answer 1

the number of protons/electrons in an atom

Question 2

mass number (atomic mass) =

Answer 2

the number of protons + the number of neutrons

Question 3

what makes up the nucleus of the atom ?

Answer 3

the protons and the neutrons

Question 4

what orbits the atom ?

Answer 4

electrons

Question 5

what happens when an atom gains/loses electrons ?

Answer 5

it is no longer called on atom

it has a positive or negative charge

Question 6

what is an ION ?

Answer 6

a positively or negatively charged atom

Question 7

what do all ions have ?

Answer 7

a full outer shell (octet rule)

Question 8

do atoms have a charge ? do ions have a charge ?

Answer 8

atoms are neutral

ions have an electric charge

Question 9

what is the purpose of chemical reactions ?

Answer 9

to achieve a full outer shell of electrons (the octet rule)

Question 10

when an atom reacts with another atom, it will either

Answer 10

lose electrons
gain electrons
share electrons to form a stable molecule

Question 11

what is an atom that has lost its electrons ?

Answer 11

a cation

Question 12

what is an atom that has gained electrons ?

Answer 12

an anion

Question 13

what are ISOTOPES ?

Answer 13

atoms with the same # of protons and electrons but have a different number of neutrons

Question 14

what is ISOTOPIC ABUNDANCE ?

Answer 14

the relative amount in which each isotope is present in an element

Question 15

what is AVERAGE ATOMIC MASS ?

Answer 15

the average of the masses of all the element’s isotopes

this is the mass found on the periodic table

Question 16

how do you calculate isotopic abundance ?

Answer 16

let x represent the abundance of one isotope, let x-1 represent the abundance of the other isotope
multiply the mass unit by the variable and add them together

Question 17

how do you calculate average atomic mass ?

Answer 17

multiple the mass by the abundance of each isotope and add them together

Question 18

the number of protons/electrons increases as we move…

Answer 18

along the row (from left to right)

Question 19

what happens to the size of the atom when we move along the row ? why ?

Answer 19

the size decreases
the strength of the attraction between the nucleus and the electrons increases
this pulls the electrons closer to the nucleus

Question 20

the number of orbitals increases as we move…

Answer 20

down a column (from top to bottom)

Question 21

what happens if the number of orbitals increase ?

Answer 21

the electrons are further from the nucleus

Question 22

what happens to the size of the orbitals as the number of rings increase ?

Answer 22

the size will increase too

Question 23

large radius = ___ ionization energy

Answer 23

low ionization energy

Question 24

small radius = ____ ionization energy

Answer 24

high ionization energy

Question 25

what is IONIZATION ENERGY ?

Answer 25

the energy that is required to remove an electron from an atom (making a positive ion/ cation)

Question 26

what is FIRST IONIZATION ENERGY ?

Answer 26

the amount of energy required to remove the weakest-held electron from a neutral atom

Question 27

the more _____ an atom holds its outermost electron, the more ______ is needed to remove an electron and the higher the I.E.

Answer 27

tightly | energy

Question 28

what happens to the attraction between the nucleus and electrons as you go across a period ?

Answer 28

the attraction in the outer energy level increases

Question 29

is the I.E. high or low when it takes more energy to remove an electron ?

Answer 29

the I.E. is higher

Question 30

is it easy to remove electrons when the I.E. is high ?

Answer 30

no | it is easier to remove when the I.E. decreases

Question 31

is it easy to remove electrons when the I.E. is low ?

Answer 31

yes

Question 32

what happens to the attraction between the nucleus and electrons as you go down a column ?

Answer 32

the attraction decreases since the electrons are further from the force of the nucleus

Question 33

the removal of a second and third electron is progressively more difficult. Why ?

Answer 33

the removal of an electron causes a reduced radius of an atom the reduced radius strengthens the attraction between the nucleus and the electrons therefore, the removal of another electron is more difficult

Question 34

what is ELECTRON AFFINITY ?

Answer 34

the energy that is released when an atom gains an electron to form an anion

Question 35

what happens to the atom when energy is released from it ?

Answer 35

the atom becomes more stable

Question 36

what does a high EA mean ?

Answer 36

the addition of one electron releases a large amount of energy

Question 37

greater nuclear attraction =

Answer 37

smaller atom | greater EA

Question 38

what happens to EA when you go down a column ?

Answer 38

the EA decreases as atoms get larger

Question 39

what happens to EA when you move across the period

Answer 39

EA increases as atoms get smaller

Question 40

are electrons always shared equally between atoms ? why ?

Answer 40

not always | because each element has a different attraction for the bonding pairs of electrons

Question 41

what is ELECTRONEGATIVITY ?

Answer 41

measure of the relative attraction of an atom for the bonding electrons

Question 42

what does a high EN mean ?

Answer 42

the atom has a high attraction for bonding electrons (likely to gain electrons)

Question 43

what does a low EN mean ?

Answer 43

the atom is likely to lose electrons

Question 44

what element has the strongest attraction of electron pairs ?

Answer 44

fluorine

Question 45

what does the difference in electronegativity determine ?

Answer 45

the type of intramolecular bond between 2 atoms