Brainscape's Knowledge GenomeTM

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


See full index

IB Chemistry SL > Periodicity > Flashcards

Periodicity Flashcards

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

what is periodicity

A

the regular reputation of properties of elements arising from patterns in their electron arrangement

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

how are elements arranged in the periodic table

A

according to their increasing atomic number and the number of protons

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

what are the 4 blocks

A

s p d f

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

why is Zn not a transition metal

A

because it does not form complete ions with incomplete d sub levels

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

what is atomic radii

A

the distance from the nucleus the the outermost electrons

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

how is atomic radii defined

A

as half the distance between the nuclei of two bonded atoms of the same element

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

atomic radii trend

A

Helium has the smallest atomic radii

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

why does atomic radii increase down a group

A

because the electron becomes further away from the nucleus

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

why does atomic radii decrease across a period

A

due to the increasing number of protons that pull the electrons in more tightly

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

what is ionic radius

A

the radius of an atom ion obtained by adding the distance between two ions and adding the ionic radius of the cation and anion

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

what is a cation

A

the positive ion

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

what is an anion

A

the negative ion

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

cations + ionic radius

A

positive ions radii are smaller than that of their parent atoms

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

anions + ionic radius

A

negative ions radii are bigger than that of their parent atoms

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

way of remembering size order of cation anion and atom

A

cation

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

ionic radius trend down a group

A

cation + anion INCREASE as outer level gets further away from nucleus

17
Q

ionic radius trend across a period

A

CATIONS: ionic radii decrease due to the increasing number of protons

ANIONS: decrease of atomic radii, but the electrons remain the same for the anions

18
Q

what is the first ionization energy

A

the energy required to remove one mole of electrons from one mole of gaseous atoms

19
Q

ionization energy trend down a group

A

DECREASES due to the increased distance between the nucleus + outer energy level that reduces the force of attraction between the nucleus and outer electrons

20
Q

ionization energy trend across a period

A

INCREASES due to the the increase in effective nuclear charge that causes electrons to be held more tightly

21
Q

what is electron affinity

A

the energy change when one mole of electrons is added to one mole of gaseous atoms to form on mole of gaseous ions

x + e- = x-

22
Q

electron affinity ACROSS PERIOD:

A

increases due to the increase in nucleus charge

23
Q

electron affinity trend

A

F has the highest electron affinity

24
Q

what is electronegativity

A

its the measure of attraction of a nucleus to bonding electrons

25
Q

electronegativity trend

A

F has the highest electronegativity

26
Q

electronegativity trend across a period

A

INCREASE from left to right due to the increase in nuclear charge

27
Q

electronegativity trend down a group

A

decrease as electrons move further away from the nucleus

28
Q

melting point trend down group 1

A

decreases

29
Q

melting point trend down group 17

A

increases

30
Q

period 3 oxide trend

A

oxides change from basic to amphoteric to acidic across a period

31
Q

acidic oxides reaction

A

react with water to produce acidic solutions

32
Q

basic oxide

A

react with water to form salt and water

33
Q

bonding trend

A

left to right: ionic to covalent

34
Q

group 17 trend

A

reactivity decreases down the group

35
Q

group 1

A

reactivity increases down a group

36
Q

boilin gpoint trend

A
  1. increase due to intermolecular forces
  2. increase due to number of carbons attached
  3. DECREASE due to branching

IB Chemistry SL (7 decks)

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