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Cphm Midterm > Chem > Flashcards

Chem Flashcards

1
Q

It helps us understand the composition of molecules and they form bonds.

A

Lewis structure

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2
Q

The shape of a molecule is determined by its _________, the angles made by the lines joining the nuclei of the atoms in the molecule.

A

Bond angles

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3
Q

The bond angles of a molecule, together with the _______ define the shape and size of the molecule.

A

bond lengths

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4
Q

It gives information about the general shape of the molecule as well as bond lengths, bond angles, torsional angles and any other geometrical parameters that determine the position of each atom.

A

Molecular geometry

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5
Q

In ________ the bonds are of directional nature because the shared pairs of electrons remain localized in a definite space between the nuclei of the participating atoms.

A

covalent molecules

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6
Q

It used to predict the molecular geometry of a molecule when both bonding and nonbonding pairs are present in the molecule.

A

VSEPR model or Valence Shell Electron Pair Repulsion

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7
Q

The arrangement of electron domains about the central atom of a molecule or ion is called ________?

A

electron-domain geometry

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8
Q

We can use the VSEPR model to predict the geometry of most polyatomic molecules and ions by focusing only on the number of electron pairs around the _______?

A

Central atom

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9
Q

According to this model, valence electrons
in the Lewis structure form _______, which may consist of a __________, a ________, a ______, a lone pair of electrons, or even a single unpaired electron, which in the VSEPR model is counted as a lone pair.

A

Group
Single bond
Double
Triple bond

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10
Q

A bonding pair of electrons thus defines a region in which the electrons are most likely to be found. We will refer to such a region as an ______ .

A

Electron domain

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11
Q

What are two types of electron domains:

A

1) A bonded atom
2) A non-bonding pair of electrons

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12
Q

Note

A

The VSEPR model can predict the structure of nearly any molecule
or polyatomic ion in which the central atom is a nonmetal, as well as the structures of many molecules
and polyatomic ions with a central metal atom. The premise of the VSEPR theory is that electron pairs located in bonds and lone pairs repel each other and will therefore adopt the geometry that places electron pairs as far apart from each other as possible. This theory is very simplistic and does not account for the subtleties of orbital interactions that influence molecular shapes; however, the simple VSEPR counting procedure accurately predicts the three-dimensional structures of a large number of compounds, which cannot be predicted using the Lewis electron-pair approach.

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13
Q

Note

A

Each multiple bond in a molecule also constitutes a single electron domain. Each nonbonding pair, single bond, or multiple bond produces a single electron domain around the central atom in a molecule.

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14
Q

Note

A

.
Using the VSEPR model, the molecular geometry can be determined when there is nonbonding electron present in the central atom.

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15
Q

What are the two types of attraction?

A

Intramolecular forces of attraction
Intermolecular forces of attraction

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16
Q

What attraction that within inside the molecule?

A

Intramolecular forces of attractione

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17
Q

What attraction that is between the molecule?

A

Intermolecular forces of attraction

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18
Q

Intermolecular forces of attraction have two bonding. What are those bonding?

A

Ionic bonding
Covalent bonding

19
Q

What is ionic bonding?

A

Transfer of electrons

20
Q

What is covalent bonding?

A

Sharing of electrons

21
Q

What are the two types of covalent bonding?

A

Polar covalent bonding
Non polar covalent bonding

22
Q

Electron shared UNEQUALLY

A

Polar Covalent bonding

23
Q

Electron shared EQUALLY

A

Non polar covalent bonding

24
Q

There are 4 types of intermolecular forces of attraction. What are those?

A

Hydrogen bond
Ion-dipole
Ion induced dipole
Van der Waals

25
Q

What are the 4 parts of Van der Waals?

A

London Dispersion
Debye
Keesom

26
Q

It is the Attraction of Hydrogen Atom to a highly electronegative atoms (F, O, N).

A

Hydrogen Bond

27
Q
  • is an intermolecular force (IMF) that forms a special type of _________ _____ attraction when a hydrogen atom bonded to a strongly electronegative atom exists in the vicinity of another electronegative atom with a lone pair of electrons.
A

Dipole dipole

28
Q

intermolecular force of attraction between a charge ion (cation or anion) and a molecule. It is found commonly in the solution where ionic compounds dissolve in polar solvents.

A

Ion-dipole

29
Q

contains unequal number of protons and electrons.

A

Ion

30
Q

contains 2 charges, where one side is positive (+), and the other is negative (-)

A

Dipole

31
Q

When an ion is placed next to a non-polar molecule, the ion forced it to be dipole.
The dipole is TEMPORARY

A

Ion-induced dipole

32
Q

force that is a weak attraction that results when an ion interacts with a nonpolar molecule The ion disturbs the arrangement of electrons in the nonpolar molecule, causing it to form a temporary dipole.

A

Ion-induced dipole

33
Q

-Force of attraction between a non-polar, and non-polar molecule. - Weakest force
- aka: Induced-Dipole – Induced-Dipole Interaction

A

London Dispersion

34
Q

is defined as the attraction between a polar molecule and a nonpolar molecule, which governs many self-assembling processes in materials.
- always attractive; does not vanish with higher temperature
- permanent (dipole – induced dipole)
- aka: Dipole-induced dipole interaction

A

DEBYE

35
Q

-attrraction between a polar and a polar molecule.
- are the electrostatic forces between two permanent polar molecules. Generally, the positive end of one molecule is attracted to the negative end of another molecule. As a result, the two molecules come closer, adding to the stability of the substance. This interaction is different from a regular ionic or covalent bond since there is no transfer or sharing of electrons.
- aka: Dipole-Dipole Interaction

A

Keesom

36
Q
  • a measure of how equally the electrons in a bond are shared between the atoms of the bond.
A

Bond polarity

37
Q

It was defined as the ability of an atom in a molecule or an ion to attract electrons to itself.

A

Electronegativity

38
Q

A bond is nonpolar if the bonded atoms have ______ electronegativities.

A

Equal

39
Q

If the electronegativities of the bonded atoms are ________, the bond is polarized toward the more electronegative atom.

A

Not equal

40
Q

Bonding electron shared equally between two atom. No charges on atom.

A

Non-polar covalent bonding

41
Q

Bonding of electron shared unequally between two atoms.partial charges of ion.

A

Polar covalent bonding

42
Q

Complete transfer of one or more valence electron. Full charges pf resulting ion.

A

Ionic bond

43
Q

Note

A

Bond dipoles and dipole moments are vector quantities; that is, they have both a magnitude and a direction. The dipole moment of a polyatomic molecule is the vector sum of its bond dipoles. Both the magnitudes and the directions of the bond dipoles must be considered when summing

Cphm Midterm (14 decks)

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