Chemical Bonding and Molecular Structure

Question 1

What are the physical properties used to replace damaged tissue?

Answer 1

strength, durability, polarity

Question 2

this is the nature of electrical charges on surfaces

Answer 2

polarity

Question 3

this is the ability of material to interact biologically without triggering an immune response

Answer 3

biocompatibility

Question 4

the greater the difference in metallic/nonmetallic properties, the more likely it is a compound will be ___

Answer 4

ionic

Question 4

this is formed by the electrostatic attraction of oppositely charged ions

Answer 4

ionic bond

Question 5

Ionic compounds form __ and __.

Answer 5

metals and nonmetals

Question 6

In the formation of cations with np6 electronic configuration, metals in the s and p blocks have __ ionization energies.

Answer 6

low

Question 7

large jumps in ionization energy occur when ____ an electron from an np6 electronic configuration

Answer 7

removing

Question 8

these are smaller than their corresponding neutral atoms

Answer 8

cations

Question 9

___ electrons reduces electron electron repulsion

Answer 9

losing

Question 10

remaining electrons are ____ bound to the nucleus

Answer 10

more tightly

Question 11

these can form cations with more than one possible charge

Answer 11

transition metals

Question 12

they first lose electrons from the s subshell

Answer 12

transition metals

Question 13

common example of ions that are stable

Answer 13

Fe^2+ and Fe^3+

Question 14

in the formation of anions with an np6 electronic configuration, ___ have negative electron affinities

Answer 14

nonmetals

Question 15

these are larger than their corresponding neutral atoms

Answer 15

anions

Question 16

___ electrons increases electron electron repulsion

Answer 16

gaining

Question 17

valence electrons are _____ bound to the nucleus

Answer 17

less tightly

Question 18

________ increases from left to right across a period

Answer 18

number of protons

Question 19

____ decrease in size from left to right across the periodic table

Answer 19

cations and anions

Question 20

____ are held more tightly from left to right across a period, resulting in smaller ions

Answer 20

electrons

Question 21

energy input to form the cation is _____ by energy released by forming the anion.

Answer 21

not offset

Question 21

electron affinites for nonmetals are _____

Answer 21

negative

Question 21

forming an ionic bond between a ___ and ___ usually required energy

Answer 21

metal and nonmetal

Question 22

ionization energies are _____

Answer 22

positive

Question 23

once an ion pair is formed, _________ between the ions significantly lowers overall energy

Answer 23

electrostatic force of attraction

Question 24

in formation of ions, what is the formula for Force? (coulomb's law)

Answer 24

F=q1*q2/r^2

Question 25

using potential energy (V), the ion pair can be calculated with what formula?

Answer 25

V = k*(q1*q2/r)

Question 26

what is the value or k in V = k*(q1*q2/r)

Answer 26

1.389x10^5 kJ pm/mol

Question 27

in ionic solids, the ions are arranged in a ____

Answer 27

crystal lattice

Question 28

strength of interaction ____ with distances

Answer 28

decreases

Question 28

Ions experience attractive and repulsive interactions in _______

Answer 28

three dimensions

Question 28

is the overall result of the attractive and repulsive forces a crystal contains

Answer 28

lattice energy

Question 29

form ionic compounds with small lattice energies.

Answer 29

Large ions with small charges

Question 29

is based on the sharing of pairs of electrons between two atoms.

Answer 29

covalent bond

Question 29

form ionic compounds with large lattice energies.

Answer 29

Small ions with large charges

Question 30

what is the Driving force behind bond formation?

Answer 30

lowering of overall energy.

Question 31

_______ lowers energy by transferring electrons between a metal and a nonmetal.

Answer 31

Ionic bonding

Question 32

Electrons on each atom are ______ to the nucleus of the other atom

Answer 32

attracted

Question 32

lowers energy by sharing electrons between two nonmetals.

Answer 32

Covalent bonding

Question 33

forms where the attractive and repulsive forces balance each other and energy is at a minimum.

Answer 33

covalent bond

Question 33

Nuclei of the bonding atoms _____ each other, as do the bonding electrons.

Answer 33

repel

Question 34

energy released when isolated atoms form a covalent bond.

Answer 34

Bond energy

Question 35

vary depending on the bonding atoms involved.

Answer 35

bond energies

Question 35

an atom will form covalent bonds to achieve a complement of eight valence electrons

Answer 35

octet rule

Question 35

the distance between the nuclei of the bonding atoms where the potential energy is a minimum.

Answer 35

Bond length

Question 35

Formation of bonds always releases _______

Answer 35

energy

Question 36

Once a bond is formed, the same amount of energy. what is this energy?

Answer 36

bond energy

Question 37

are u happy

Answer 37

no

Question 38

The valence shell electronic configuration is ______ for a total of eight electrons.

Answer 38

ns2np6

Question 39

these keep track of valence electrons, especially for main group elements, allowing prediction of bonding in molecules

Answer 39

lewis dot symbols

Question 40

it shows how electrons are shared in a molecule

Answer 40

Lewis dot Structures

Question 41

lagi

Answer 41

lagi

Question 42

pairs of electrons associated with one atom are called ______

Answer 42

nonbonding or lone pair electrons

Question 43

A pair of shared electrons between two atoms is called

Answer 43

bonding pair

Question 44

this bond results when two bonding pairs are shared

Answer 44

double bond

Question 45

this bond results when three bonding pairs are shared

Answer 45

triple bond

Question 46

Strength of the covalent bond increases as the ____ increases

Answer 46

number of bonding pairs

Question 47

the attraction of an atom for the shared electrons in a covalent bond

Answer 47

electronegativity

Question 48

Electronegativities increase from _____ across a period and from ______ for a group

Answer 48

left to right, bottom to top

Question 48

this element is the most electronegative element, with how much electronegativity?

Answer 48

Fluorine, 4.0

Question 48

is not shared equally when elements with different electronegativities bond

Answer 48

Electron density

Question 49

The more electronegative element experiences an increase in electron density and attains a ________

Answer 49

partial negative charge

Question 50

The less electronegative element experiences a decrease in electron density and attains a ________

Answer 50

partial positive charge

Question 51

The two points of positive and negative charge constitute a _____

Answer 51

dipole

Question 52

A bond along which a dipole exists

Answer 52

polar bond

Question 53

polar bond is also called

Answer 53

polar covalent bond

Question 54

The greater the electronegativity difference, the ____ polar bond

Answer 54

more

Question 55

When the electronegativity difference is zero, the bond is classified as

Answer 55

nonpolar covalent

Question 56

When the electronegativity difference exceeds 2.0, the bond is classified as

Answer 56

ionic

Question 57

indicate how many bonds are formed and between which elements in a compound

Answer 57

lewis structures

Question 58

this structures can be drawn when the choice of multiple bond location is arbitrary.

Answer 58

resonance structures

Question 59

in resonance structures, position of all atoms are _____; only the positions of the electrons are different

Answer 59

identical

Question 60

this indicates the structures are resonance structures.

Answer 60

double arrow

Question 61

is the result of constructive interference for end-to-end overlap, where electron density lies along a line between the bonding atoms.

Answer 61

sigma bond

Question 62

is the result of constructive interference for side- to-side overlap, where electron density lies above and below, or in front and in back of a line between the bonding atoms

Answer 62

pi bond

Question 63

reconciles the notion of orbital overlap with observations of molecular shapes and structures

Answer 63

Orbital Hybridization

Question 64

is the way bonded atoms arrange themselves in three dimensions

Answer 64

molecular shape

Question 65

in this theory, molecules assume a shape that allows them to minimize the repulsions between electron pairs in the valence shell of the central atom

Answer 65

valence shell electron pair repulsion (VSEPR)

Question 66

what is the angle of linear and number of electron pairs?

Answer 66

180, 2 electron pairs

Question 67

what is the angle of trigonal planar and number of electron pairs?

Answer 67

120, 3 electron pairs

Question 68

what is the angle of tetrahedral and number of electron pairs?

Answer 68

109.5, 4 electrons pairs

Question 69

what is the angle of trigonal bipyramidal and number of electron pairs?

Answer 69

120 or 90, 5 electron pairs

Question 70

what is the angle of octahedral and number of electron pairs?

Answer 70

90 or 180, 6 electron pairs

Question 71

these may offer a promising route for drug delivery, since they can deliver drugs to a targeted location and thus avoid side effects from affecting non-targeted organs.

Answer 71

Mesoporous silica nanoparticles