Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHEMISTRY unit 1 > chapter 1 > Flashcards

chapter 1 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

atomic # =

A

the number of protons/electrons in an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

mass number (atomic mass) =

A

the number of protons + the number of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what makes up the nucleus of the atom ?

A

the protons and the neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what orbits the atom ?

A

electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what happens when an atom gains/loses electrons ?

A

it is no longer called on atom

it has a positive or negative charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what is an ION ?

A

a positively or negatively charged atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what do all ions have ?

A

a full outer shell (octet rule)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

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

A

atoms are neutral

ions have an electric charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what is the purpose of chemical reactions ?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

when an atom reacts with another atom, it will either

A

lose electrons
gain electrons
share electrons to form a stable molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what is an atom that has lost its electrons ?

A

a cation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what is an atom that has gained electrons ?

A

an anion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what are ISOTOPES ?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what is ISOTOPIC ABUNDANCE ?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what is AVERAGE ATOMIC MASS ?

A

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

this is the mass found on the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

how do you calculate isotopic abundance ?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

how do you calculate average atomic mass ?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

the number of protons/electrons increases as we move…

A

along the row (from left to right)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

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

A

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

20
Q

the number of orbitals increases as we move…

A

down a column (from top to bottom)

21
Q

what happens if the number of orbitals increase ?

A

the electrons are further from the nucleus

22
Q

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

A

the size will increase too

23
Q

large radius = ___ ionization energy

A

low ionization energy

24
Q

small radius = ____ ionization energy

A

high ionization energy

25
Q

what is IONIZATION ENERGY ?

A

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

26
Q

what is FIRST IONIZATION ENERGY ?

A

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

27
Q

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

A

tightly

energy

28
Q

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

A

the attraction in the outer energy level increases

29
Q

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

A

the I.E. is higher

30
Q

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

A

no

it is easier to remove when the I.E. decreases

31
Q

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

A

yes

32
Q

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

A

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

33
Q

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

A

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

34
Q

what is ELECTRON AFFINITY ?

A

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

35
Q

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

A

the atom becomes more stable

36
Q

what does a high EA mean ?

A

the addition of one electron releases a large amount of energy

37
Q

greater nuclear attraction =

A

smaller atom

greater EA

38
Q

what happens to EA when you go down a column ?

A

the EA decreases as atoms get larger

39
Q

what happens to EA when you move across the period

A

EA increases as atoms get smaller

40
Q

are electrons always shared equally between atoms ? why ?

A

not always

because each element has a different attraction for the bonding pairs of electrons

41
Q

what is ELECTRONEGATIVITY ?

A

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

42
Q

what does a high EN mean ?

A

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

43
Q

what does a low EN mean ?

A

the atom is likely to lose electrons

44
Q

what element has the strongest attraction of electron pairs ?

A

fluorine

45
Q

what does the difference in electronegativity determine ?

A

the type of intramolecular bond between 2 atoms

CHEMISTRY unit 1 (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions