Brainscape's Knowledge GenomeTM

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


See full index

Chem Unit 7, 8, 9 > Ch. 7,8,9 Test > Flashcards

Ch. 7,8,9 Test Flashcards

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

Naming covalent compounds

Prefix for 1

A

Mono

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

Naming covalent compounds

Prefix for 2

A

Di

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

Naming covalent compounds

Prefix for 3

A

Tri

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

Naming covalent compounds

Prefix for 4

A

Tetra

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

Naming covalent compounds

Prefix for 5

A

Penta

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

Naming covalent compounds

Prefix for 6

A

Hexa

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

Naming covalent compounds

Prefix for 7

A

Hepta

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

Naming covalent compounds

Prefix for 8

A

Octa

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

Naming covalent compounds

Prefix for 9

A

Nona

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

Naming covalent compounds

Prefix for 10

A

Deca

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

Chemical Bond

A

The force holding atoms together in a compound or molecule

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

Types of Bonds

A

Ionic
Covalent (polar/nonpolar)
Metallic

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

Octet Rule

A

Atoms tend to lose or gain electrons to obtain the same electron configuration as a noble gas

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

Cations

A

Atoms who lose electrons
Metals
Positive Charge

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

Anions

A

Atoms that gain electrons
Nonmentals
Negative Charge

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

Ionic Bond

A

The electrostatic forces that bring a cation and anion together.
A transfer of electrons that results in a positive and negative ion

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

Ionic Bonds … Known as..

A

Salts

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

Ionic bond electronegativity is …

A

greater than two

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

Properties of ionic compounds

A

Soluble in water
Conduct electric current in molten or soluble state
High melting points

20
Q

Metallic Bonds

A

form when metal atoms crowd together and valence shells overlap

21
Q

Valence electrons in metallic bonds

A

Become “delocalized”

Like a “sea of electrons” flowing through positively charged metal ions

22
Q

Properties of metals

A

Conduct electricity
Malleable and ductile
Insoluble

23
Q

Ions

A

charged particles

24
Q

Monatomic Ion

A

formed when a single atom has gained or lost electrons

25
Q

Polyatomic Ion

A

When a group of atoms collectively has a charge

26
Q

Multivalent Ions

A

Transition Metals

Uses stock system to name (indicated by Roman Numeral)

27
Q

Exceptions to multivalent roman numeral rule

A

Silver +1
Zinc +2
Scandium +3
Cadmium +2

28
Q

Naming Binary Compounds

A

Cation named first, anion named second (ending in -ide)

29
Q

Naming Multivalent Binary Compounds

A

Criss cross method, make it so the ion is neutral

Put Roman Numeral in name

30
Q

Single covalent bonds

A

two atoms are held together by sharing a pair of electrons

1 covalent bond = 1 shared pair

31
Q

all halogens form ____________ bonds

A

single covalent

32
Q

unshared pair

A

pair of valence electrons that is not shared between atoms
do not connect 2 atoms together
“lone pair of electrons”

33
Q

strongest bond

A

triple

34
Q

VSEPR Theory

A

Repulsion between electron pairs causes molecular shapes to adjust so that the valence-electron pairs stay as far apart as possible

35
Q

Molecule with electronegativity of 0.0-0.4

A

Nonpolar covalent

36
Q

Molecule with electronegativity of 0.4-2.0

A

Polar covalent

37
Q

Molecule with electronegativity larger than 2.0

A

Ionic

38
Q

If a molecule is symmetrical.,,,

A

It is a nonpolar molecule

39
Q

If a molecule is NOT symmetrical…

A

It is a polar molecule

40
Q

Naming acids where the molecule ends in -ide

A

hydro_____ic + acid

41
Q

Naming acids where the molecule ends in -ate

A

_____ic + acid

42
Q

Naming acids where the molecule ends in -ite

A

______ous + acid

43
Q

Ionic compounds exist as ______ at room temperature

A

solids

44
Q

Properties of a covalent compound

A

low melting and boiling point, not conductors, insoluble

45
Q

polar bond

A

electrons unequally shared

46
Q

nonpolar bond

A

electrons equally shared

47
Q

Diatomic Molecules

A

H2, O2, N2, Cl2, Br2, I2, F2

Chem Unit 7, 8, 9 (2 decks)

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