Brainscape's Knowledge GenomeTM

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


See full index

AP Chem > Chapter 8- Chemical Bonding > Flashcards

Chapter 8- Chemical Bonding Flashcards

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

Ionic

A

Metals and nonmetals

Unfair sharing of electrons

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

Covalent

A

Nonmetals and nonmetals
Fair sharing of electrons
Can be polar or nonpolar

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

Metallic

A

E cloud bonds atoms

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

Octet rule

A

Atoms tend to lose or gain until they are surrounded by 8 electrons except H which needs two

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

Polar bonds

A

Covalent bonds in which electrons are shared unequally die to the differences in the elements electronegativities

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

Polar molecule (dipole)

A

A molecule containing a polar bond which results in an uneven distribution of electrons

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

Dipole moment

A

Measurement of the magnitude of dipole

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

Reasonable structures

A

Molecules with more than one plausible structure

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

Lattice energy (Eel)

A

Energy required to completely separate 1 mol of an ionic crystal into its gaseous ions

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

All ionic compounds

A

Are solid and exist as a crystal lattice

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

Ionic bonds are ______ than covalent bonds

A

Stronger

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

Formula for lattice energy

A

Eel = (constant times charges of ions) / distance between nuclei

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

Lattice energy

A

All about charge and attraction

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

Formal charge

A

The charge that an atom in a molecule would have if all of its bonding electron pairs were shared equally between atoms
(Allows us to predict correct form of a molecule)

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

Formal charge adds up to

A

The charge of the ion

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

Halogens only form

A

Single bonds

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

Anything form the throw period down can

A

Hybridize

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

Heat of reaction

A

Bonds broken-bonds formed

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

VSEPR

A

Valance shell electron pair repulsion theory

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

Electron pairs on a central atom

A

Bonded or unbounded will repel, thus creating the molecules shape

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

Electron domains

A

The areas where the electrons are likely to be located

22
Q

Electron domain geometry

A

Shape created by the electron domains

23
Q

Molecular geometry

A

The shape created by the arrangement of atoms

24
Q

Shape of two electron domains

A

Linear (180 degrees)

25
Q

Shape of three electron domains

A 
Trigonal planar (120)
Bent(120) (one unbounded pair)
26
Q

Shape of four electron domains

A 
Tetra hedral (109)
Trigonal pyramidal (107)
Bent (two unbounded electrons) (104)
27
Q

Tetrahedral

A

109

28
Q

Trigonal pyramidal

A

107

29
Q

Bent (one unbounded electron pair)

A

120

30
Q

Bent (two unbounded electron pairs)

A

104

31
Q

Trifocals planar

A

120

32
Q

How does a bond affect a molecules polarity

A

A polar bond “bond dipole” is a vector quantity. Therefore it has magnitude and direction

33
Q

Bonding site

A

Orbital with only one electron in it

34
Q

Valance bond theory

A

Covalent bonds are formed by overlapping atomic orbitals which contain electrons

35
Q

Does orbital overlap happen in polyatomic molecules?

A

Yes but the atomic orbitals (s,p,d) mix to form a hybrid orbital

36
Q

Linear

A

Sp

37
Q

Trifocals planar

A

Sp2

38
Q

Tetrahedral

A

Sp3

39
Q

Covalent bonds can be classified as

A

Sigma or pi bonds

40
Q

Sigma bond

A

End to end overlap of atomic orbitals

41
Q

The electron density of sigma bonds

A

Is concentrated along a line that connects the nuclei

42
Q

Pi bond

A

A side by side overlap of Unhybridized atomic orbitals

43
Q

Electron density of pi bonds

A

Is concentrated above and below a line that connects the nuclei

44
Q

Single bond

A

Sigma bond

45
Q

Double bond

A

One sigma

One pi

46
Q

Triple bond

A

One sigma

Two pis

47
Q

Electronic geometry may be different from molecular geometry because

A

The electronic geometry refers to how the electrons are arranged, but the molecular geometry indicates the net shows of the molcule

48
Q

VSEPR theory is based on

A

Minimization of repulsion among valance electron pairs

49
Q

The central atom in compounds with square planar geometric always abet the octet rule

A

True

50
Q

Large electronegativities difference affects molecular properties

A

By making boss stronger and shorter

Makes bonds highly polar

Makes molecule highly polar if molecular geometry permits

51
Q

Metallic bond

A

Metals and metals

Electron clouds around atom

AP Chem (12 decks)

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