Chemistry: Chemical Bonding

Front 1

a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together

Back 1

Chemical Bond

Front 2

different _____ may be of the same element or different elements

Back 2

atoms

Front 3

Atoms bond to be in a more ______ _____. They are less stable when they are __ __________. The potential energy _________ when the atoms bond.

Back 3

stable state; by themselves; decreases

Front 4

When atoms bond their _______ _________ are redistributed in ways that make the atoms more stable

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valence electrons

Front 5

The way in which the electrons are _____________ determines the type of bond

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redistributed

Front 6

chemical bonding that results from the electrical attraction between large numbers of anions and cations

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Ionic bonding

Front 7

results from the sharing of valence electron pairs between 2 atoms

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Covalent bonding

Front 8

In purely covalent bonds, the electrons are ______ _______ between the atoms

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shared equally

Front 9

Bonding between atoms of different elements is rarely ______ _____ or ______ ________

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purely ionic or purely covalent

Front 10

The bonding falls between the 2 extremes depending upon how strongly the _____ of each element attract electrons

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atoms

Front 11

(high electronegativity - low electronegativity) / * 100
high electronegativity

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% ionic character

Front 12

if % ionic character is > 50%, then an _____ bond exists

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ionic

Front 13

--if % ionic character is < 50%, then a _______ bond exists

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covalent

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a _____ ________ bond falls between 5% and 50% including 50%

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polar covalent

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a ________ ________ bond falls between 0%-5% including 5%

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nonpolar covalent

Front 16

Use the electronegativity for ___ ____ of each element to determine the % ionic character even if the compound contains more than 1 atom of an element.

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one atom

Front 17

electron configuration in which only the valence electrons are shown as dots around the element's symbol

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Electron dot Notation

Front 18

the _____ _____ _________ are not shown

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inner shell electrons

Front 19

to write electron dot notation for _______, draw the symbol with the charge on the cation

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cations

Front 20

To write the electron dot for ______, draw the symbol surrounded by 8 dots with the charge on the anion

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anions

Front 21

Chemical compounds tend to form so that each atom, by gaining, losing or sharing electrons, has an octet or 8 electrons in its highest energy level

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Octet Rule

Front 22

________ ________ _____ are covalent bonds where the electrons are shared equally by the bonded atoms resulting in a balanced distribution of electrical charge

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Nonpolar covalent bonds

Front 23

there is a ____ _____ __________ in electronegativities between the atoms

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very small difference

Front 24

_____ ________ _____ are covalent bonds with an uneven distribution of electrical charges because the bonded atoms have an unequal attraction for the shared electrons

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Polar covalent bonds

Front 25

the difference between the electronegativities is ___________

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significant

Front 26

the electrons are attracted to the more _______________ ____

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electronegative atom

Front 27

a neutral group of atoms that are held together by covalent bonds

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molecule

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molecules containing 2 atoms

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Diatomic molecules

Front 29

_ elements occur in nature as diatomic molecules

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7

Front 30

formulas for the 7 diatomic molecules are:

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

Front 31

A ________ _______ indicates the relative numbers of atoms of each kind of element in a chemical compound by using atomic symbols and numerical subscripts

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chemical formula

Front 32

_________ ________ show the types and numbers of atoms combined in a single molecule of a molecular compound

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Molecular formulas

Front 33

Lewis structures are formulas in which:
- ______ _______ represent the nuclei and inner shell electrons
- dot pairs between 2 atomic symbols represent ________ ____ in covalent bonds, dots adjacent to only one atomic symbol represent unshared electrons

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atomic symbols

Front 34

__________ _______ indicates the kind, number, arrangement and bonds but not the unshared pairs of electrons in the atoms in a molecule

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structural formula

Front 35

covalent bonds produced by the sharing of one pair of electrons between 2 atoms

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single bonds

Front 36

covalent bonds produced by the sharing of 2 pairs of electrons between 2 atoms.

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double bonds

Front 37

covalent bonds produced by the sharing of 3 pairs of electrons between 2 atoms

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triple bonds

Front 38

Compounds made of positive and negative ions combined so that the numbers of positive and negative charges are equal

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Ionic compounds

Front 39

The simplest collection of atoms from which an ionic compound's formula can be established

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Formula units

Front 40

_______ _____ are not independent neutral units that can be separated and examined like a molecule can be

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formula units

Front 41

_____ _________ are networks of positive and negative ions mutually attracted to each other

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ionic compounds

Front 42

_______ ____ represents the lowest ratio of the compound's combined ions that give electrical neutrality

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formula unit

Front 43

ionic compounds usually exist as ___________ _____

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crystalline solid

Front 44

_______ _______ is the orderly arrangement of ions in an ionic compound

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crystal lattice

Front 45

In naming ______, the ending of the element's name is replaced with "ide"

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anions

Front 46

It creates the ability for metals to be ____ __________ __ ___________ in the solid state

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good conductors of electricity

Front 47

within a metal, there are usually 1 or 2 electrons in the outer s-sublevel with no electrons in the _____ _-________

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outer p-sublevel

Front 48

the vacant sublevels overlap providing a path for the _______ _________ to move throughout the metal

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valence electrons

Front 49

the attraction between the metal's atoms and the surrounding sea of electrons

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metallic bonding

Front 50

good conductors of heat and electricity because the sea of electrons carries the ____ or ___________ throughout the atoms

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heat or electricity

Front 51

_____ because metals absorb light at different frequencies resulting in electron transition

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Shiny

Front 52

The shine is the light given off as the electrons return to the ______ _____

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ground state

Front 53

_________ and _______ because metallic bonding is the same in all directions

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Malleable and ductile

Front 54

forces that hold the different molecules in a substance together

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Intermolecular forces

Front 55

Three types of intermolecular forces:

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- dipole-dipole
- hydrogen bonding
- London dipersion forces

Front 56

forces of attraction between polar molecules

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Dipole-dipole

Front 57

negative region in one polar molecule attracts the ________ ______ in an adjacent molecule throughout the substance

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positive region

Front 58

short range forces acting on nearby _________

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molecules

Front 59

important in determining ________ __________ such as the boiling point of a substance or its solubility

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physical properties

Front 60

special type of dipole-dipole force that is very strong

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Hydrogen bonding

Front 61

occurs in compounds containing _-_ bonds, _-_ bonds and _-_ bonds

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H-F; H-O; H-N

Front 62

hydrogen atoms that are bonded to a highly electronegative atom are attracted to an ________ ____ __ _________ of a highly electronegative atom in a nearby molecule

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unshared pair of electrons

Front 63

temporary dipoles that occur in any polar or nonpolar molecule

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London dispersion forces

Front 64

occur because the electrons are __________ ______

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constantly moving

Front 65

at any moment the electron distribution in the electron cloud becomes ______, thus creating a dipole

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uneven

Front 66

these temporary _______ induce dipoles in adjacent molecules and cause a weak attraction that holds the molecules together

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dipoles

Front 67

these are the only intermolecular forces acting between _____ _____ and _____ ________ _________

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noble gases and other nonpolar molecules