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Chemistry > Study Guide Lewis Structure VSEPR > Flashcards

Study Guide Lewis Structure VSEPR Flashcards

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1
Q

Define chemical bond

A

a mutual attraction between two atoms resulting from a redistribution of their outer electrons.

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2
Q

What is an ionic bond?

A

A transfer of electrons

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3
Q

What is a covalent bond?

A

A sharing of electrons

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4
Q

What is a crystalline solid?

A

A 3-d repeating pattern of + and - ions, formed by an ionic compound

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5
Q

What is a metallic bond?

A

force of attraction between valence electrons and the metal atoms. It is the sharing of many detached electrons between many positive ions

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6
Q

What is a sea of electrons?

A

instead of orbiting their respective metal atoms, they form a “sea” of electrons that surrounds the positively charged atomic nuclei of the interacting metal ions.

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7
Q

What is luster?

A

the way light interacts with the surface of a crystal, rock, or mineral.

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8
Q

What is malleability?

A

ability of a substance, usually a metal, to be deformed or molded into a different shape

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9
Q

What is conductivity?

A

measure of water’s ability to conduct electricity.

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10
Q

What is ductile?

A

a solid material’s ability to deform under tensile stress; this is often characterized by the material’s ability to be stretched into a wire

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11
Q

What is solubility

A

Measurement of a substances ability to be dissolved in water

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12
Q

What is a polar covalent bond?

A

chemical bond in which the electrons required to form a bond is unequally shared between two atoms

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13
Q

What is a non polar covalent bond?

A

a type of chemical bond where two atoms share a pair of electrons with each other.

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14
Q

What is bond length?

A

bond length or bond distance is the average distance between nuclei of two bonded atoms in a molecule.

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15
Q

What is bond strength?

A

the strength with which a chemical bond holds two atoms together

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16
Q

What is the octet rule?

A

atoms of main-group elements tend to combine in such a way that each atom has eight electrons in its valence shell

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17
Q

What is the lewis dot structure?

A

diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

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18
Q

What is a single bond?

A

a chemical bond in which one pair of electrons is shared between two atoms.

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19
Q

What is a double bond?

A

a chemical bond in which two pairs of electrons are shared between two atoms.

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20
Q

What is a triple bond?

A

a chemical bond in which three pairs of electrons are shared between two atoms.

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21
Q

What is a lone pair?

A

a lone pair refers to a pair of valence electrons that are not shared with another atom and is sometimes called a non-bonding pair

22
Q

What is a diatomic molecule?

A

composed of only two atoms, of the same or different chemical elements.

23
Q

What is electronegativity?

A

describes the tendency of an atom to attract a shared pair of electrons towards itself.

24
Q

What is bond polarity

A

Bond polarities arise from bonds between atoms of different electronegativity.

25
Q

What is molecular polarity

A

Molecular polarities that arise from the sums of all of the individual bond polarities.

26
Q

What is the VSEPR Theory?

A

Valence shell electron pair repulsion (VSEPR) theory is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms.

27
Q

What is a dipole?

A

eparation of charges within a molecule between two covalently bonded atoms.

28
Q

What is an intermolecular force?

A

forces that hold two molecules together

29
Q

What are Columbia forces?

A

Coulombic attraction is the force of attraction between positive and negative charges
- If the charges on the particles have opposite signs, the force will be one of attraction.

30
Q

What is an ion-ion force?

A

attractive force between ions with opposite charges. They are also referred to as ionic bonds and are the forces that hold together ionic compounds.
(OPPOSITE CHARGES ATTRACT)

31
Q

What is an ion-dipole force?

A

attractive force that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole.

32
Q

What is a dipole dipole interaction

A

Dipole-Dipole interactions result when two dipolar molecules interact with each other through space. When this occurs, the partially negative portion of one of the polar molecules is attracted to the partially positive portion of the second polar molecule.

33
Q

What is a dipole dipole interaction with hydrogen?

A

A hydrogen bond is a dipole-dipole force and is an attraction between a slightly positive hydrogen on one molecule and a slightly negative atom on another molecule.

34
Q

What are dispersion forces?

A

the weakest intermolecular force.v

35
Q

What is aqueous

A

Dissolvable by water

36
Q

Why do atoms combine to form compounds?

A

Atoms want to satisfy the octet rule, meaning they want to have 8 valence electrons on the outermost shell to make it stable. When it does not have 8 electrons, it is unstable, and so the ionic bond between two atoms form a molecule, making it stable.

37
Q

What is the difference between a ionic a covalent compound in terms of electrons?

A
  • Covalent compounds involve the sharing of two electrons between atoms and other covalent bonds.
  • Ionic compounds have both positive and negatively charged ions
38
Q

What is a covalent bond? Which electrons are involved in the formation of a covalent bond?

A

A bond that shares electrons. The outermost electrons are involved in the formation of a covalent bond

39
Q

What is the difference between polar and nonpolar bonds? Why are polar covalent bonds more common than nonpolar covalent bonds?

A

Polar bond: bond between atoms where electrons are shared unequally
Non-polar Bonds: Bond between atoms where electrons are shared equally.

40
Q

What group of elements satisfies the octet rule without forming compounds?

A

Noble Gases

41
Q

What are the exceptions to the octet rule? Use BCl3 and SF6 as examples.

A

Sometimes, if all surrounding atom satisfy the octet rule, and the middle atom has not, then a lone pair must be created.

42
Q

When you draw a Lewis structure, which atom is generally in the center? Why?

A

The one with the lowest electronegativity because it is the most conductive to sharing electrons/forming bonds

43
Q

If the lattice energy of compound A is greater than that of compound B, what do you
know about the bonds in the two compounds?

A

it will be more difficult to break the bonds in compound A than in compound B.

44
Q

Name and describe the three major types of chemical bonding.

A

ionic, covalent, and metallic
Ionic Bonding-Transfer of electrons
Covalent-Sharing of electrons
Metallic-Occur between the ionized atoms of metals and the sea of electrons around them

45
Q

Describe the differences between ionic and covalent compounds (look solubility, melting point, etc)

A

REFER TO CHART

46
Q

List 5 unique properties of metals

A

REFER TO CHART

47
Q

What are IMF’s?

A

Dispersion-Nonpolar compounds
Dipole Dipole-Polar compounds
Dipole Dipole-Polar compounds with hydrogen bonding

48
Q

Four different types of intermolecular forces:

A

Strong ionic attraction,Intermediate dipole-dipole forces

, dispersion forces, Hydrogen bond

49
Q

How does the strength of intermolecular forces compare with molecular bonds?

A

Molecular bonds are must stronger because they are not subject to change whereas the valence shells on intermolecular forces can alter

50
Q

Which state of matter has the strongest intermolecular forces?

A

Solids

Chemistry (9 decks)

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