Brainscape's Knowledge GenomeTM

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


See full index

AP Chemistry > H Chemistry: Unit 4 > Flashcards

H Chemistry: Unit 4 Flashcards

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

periodicity

A

study of the trends on the periodic table

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

octet rule

A

every element on the periodic table wants 8 electrons in their highest energy level(noble gas configuration) except hydrogen and helium

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

oxidation number

A

charge an atom has when it acquires an octet; the oxidation number for transitional elements vary

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

metals

A

solids and good conductors of heat and electricity

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

non-metals

A

gases and poor conductors of heat and eletricity

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

metalloid

A

moderate conductors of heat and electricity

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

group 1 elements

A

alkali metals

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

group 2 elements

A

alkaline earth metals

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

group 6 elements

A

chalcogens

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

group 7 elements

A

halogens

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

group 8 elements

A

noble gases

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

atomic radius

A

half the distance between the nuclei of 2 like atoms; measured in angstroms

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

atomic radius trend

A

increases as you move down and left

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

ionization energy

A

energy required to remove an electron from an atom; measured in volts

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

ionization energy trend

A

increases as you move up and right

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

electronegativity

A

ability of an atom to attract electrons to itself; measured in Paulings’

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

electronegativity trend

A

increases as you move up and right

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

shielding effect

A

electrons closer to the nucleus shield the outer electrons from the pull of the nucleus; increases with the number of electrons

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

shielding effect trend

A

increases as you move down and right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

ionic radius

A

size of an atom compared to the atomic radius when a atom gains or loses electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

chemical bond

A

bond between atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

ionic bond

A

electrostatic force between atoms(cation and anion); formula unit or salt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

cation

A

positive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

anion

A

negative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

properties of an ionic compound

A

1.form a crystal lattice
2.high melting and boiling points
3.salts are solid, hard, and brittle
4.form an electrolyte

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

lattice energy

A

energy required to remove an ion from a crystal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

electrolyte

A

substance that conducts electricity when dissolved

28
Q

monatomic ion

A

ion made up of one atom; everything on periodic table

29
Q

polyatomic ion

A

ion made of more than 1 atom

30
Q

an ionic compound is

A

neutral

31
Q

naming ionic compounds- cation first

A

-if the cation is an element on the periodic table, use its name
-if the cation is polyatomic, use its unique name
-if the cation is a transition metal with more than one share, use a Roman numeral to indicate its charge

32
Q

naming ionic compounds- anion second

A

-if the anion is monatomic off the periodic table, use its root name and add the suffix “-ide”
-if the anion is polyatomic, use its unique name on the periodic table

33
Q

covalent bond

A

bond between atoms where electrons are shared; molecule

34
Q

the covalent bond occurs when

A

attraction and repulsion forces are in balance

35
Q

attraction forces

A

nucleus of 1 atom attracted to the electrons of the other

36
Q

repulsion forces

A

nuclei of both atoms and the electrons of both atoms repel each other

37
Q

single covalent bond

A

sigma bond; bond between atoms where one pair of electrons are shared

38
Q

double covalent bond

A

1 sigma & 1 pi; bond between atoms where 2 pairs of electrons are shared

39
Q

pi bond

A

bond between parallel orbitals that overlap

40
Q

triple covalent bond

A

1 sigma & 2 pi; bond between atoms where 3 pairs of electrons are shared

41
Q

bond length

A

distance between bonded nuclei; the shorter the bond, the stronger it is; multiple bonds are shorter and stronger

42
Q

bond dissociation energy(BDE)

A

energy required to break a covalent bond

43
Q

diatomic gases

A

7 elements on the periodic table that exist in nature in pairs; I H N Cl O Br F

44
Q

resonance structure

A

lewis structure that can be drawn in more than one way to illustrate the sharing of a double bond; use a double arrow

45
Q

expanded octet

A

center atom will occasionally bond with empty d orbitals and have more than 8 electrons in the highest energy level(s & p)

46
Q

VSEPR(valence shell electron pair repulsion) theory

A

unshared pairs of electrons on the center atom in a lewis structure take up space

47
Q

A.X.E Notation

A

A- center atom
X- atoms that re bonded to the center atom
E- unshared pairs of electrons

48
Q

AX2

A

linear

49
Q

AX3

A

trigonal planar

50
Q

AX4

A

tetrahedral

51
Q

AX3E

A

trigonal pyramidal

52
Q

AX2E2

A

bent

53
Q

AX5

A

trigonal bipyramidal

54
Q

naming molecules- prefix method

A

prefixes indicate the number of atoms in the molecule

55
Q

naming molecules- 1

A

mono

56
Q

naming molecules- 2

A

di

57
Q

naming molecules- 3

A

tri

58
Q

naming molecules- 4

A

tetra

59
Q

naming molecules- 5

A

penta

60
Q

naming molecules- 6

A

hexa

61
Q

naming molecules- 7

A

hepta

62
Q

naming molecules- 8

A

octa

63
Q

naming molecules- 9

A

nona

64
Q

naming molecules- 10

A

deca

65
Q

naming molecules

A
  1. first element- use a prefix and its name off of the periodic table
  2. second element- use a prefix and its root name off periodic table with the “-ide” suffix
  3. omit “mono” from first element
66
Q

acid

A

substance that donates hydrogen to a solution and lowers pH; anion determines acid name

AP Chemistry (16 decks)

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