Chemistry (Bonding theory and Lewis formulas, Ionic, Moleculer, Vesper structures)

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1

Valence electrons occupying the

Highest energy level

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energy-level theory says the the electrons in lower energy levels are held so ___ by their___- that, during chemical recation, they remain__

Strongly , Nucleus, Unchanged

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( )

( ) o ( ) <----Orbital

( )

A region of space around an atoms nucleus where an electron my exist

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Valence orbitals

The volumes of space that can be occupied by electrons in a atoms highest energy level

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Bonding electrons

An atom with a valence orbital that is occupied by a single electron and therefore share that electron with another atom.

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Lone pair

A full valence orbital with two electrons which has a repeling affect on any nearby orbitals

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Quantum mechanics rules

  1. The FIRST energy level has room for only one orbital with a maximum of 2 electrons

  2. Energy levels above the first have room for FOUR orbitals which is 8 electrons max.

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Octet rule

The octet rule is a chemical rule of thumb that reflects the theory that main-group elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas

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Atoms that always obey the octet rule when bonding.

C1,N1, O1, F1

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Atoms that are exceptions to the octet rule.

NO, SF6, BCl3

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Lewis symbol also called

Lewis dot diagram

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Rules for drawing lewis symbol

  1. Write the element symbol to represent the nucleus

  2. Add a dot to represent each valence electron

  3. If more than four electrons start filling with a seconf electron

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Ionic bond

  1. electrostatic attraction between positive and negative ions

  2. Metals tend to lose the electrons well non-metals gain

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Define electronegativity

relative ability of an atom to attract a pair of bonding electrons in its valence level

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The atom with highes electronnegativivty

Fluorine (4.0)

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Atom with lowest electronegativity

Francium (0.7)

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electronnegativty range

0.7-4.0

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A generalization is that metals have ________ electronegativety while nonmetals tend to have ___ electronegativety

Low, High

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Types of bonding

Covalent, Ionic, Metallic

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  • If the electronegativities of each atom are relatively high, then neither atom “wins” the competition

  • Instead the pair of bonding electrons s shared between two atoms and a COVALENT bond forms

  • Usually occurs between two non-metal atoms (2C)

  • The electron sharing may be unequal (CO)

Covalent bonding

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  • If the electronegativities of the two atoms are very diffrent, the atom with the higher electronegativitie will “win” and take the bonding electron from the lower electronegativities

  • an ___ forms when an electron tansfer occurs

  • Occurs between metals and non-metals

  • ions arrange themselves in position where the maximum total attraction between positive and ions occur

Ionic bonding

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  • If the electronegativities of the colliding atoms are both low, then the atoms share valence electrons in a __ bond.

  • The valence electrons are not held strongly by their atoms; so they can move arround

  • there will be a large number of positive electrons surrounded by a sea of moving electrons

  • this is weak attraction in which the metal atoms are not arranged in any particular arranements, which create that is flexable, malleable, and ductile

Metallic bonding

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Scientis figured out that two non-metal atoms must ___ a pair of elctrons in a ______ bond

share, covalent bond

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Covalent bonds shares one pair of elctrons

single

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Covalent bonds shares Two pairs pair of elctrons

double

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Covalent bonds shares three pairs of elctrons

triple

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Diatomic molecules

O2, CL2, N2, H2, I2, Br2

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polyatomic molecules

P4, S8

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  • Molecular compunds do not have simplest ratio formulas like ionic compounds

  • Instead, molecular formulas show the actual number and arrangment of the atoms

  • all atomsb strive to fill their valence orbitals with a full octet

  • Bonding capacity = max # of single covalent bonds

  • in turn, the # of ___ determine an atoms bonding capacity

Bonding electrons

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Coordinate covalent bond

Covalent bond in which pne pf the atoms donates BOTH electrons

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o oo

o C o o F o o

o oo

lewis

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C-F=H

Structural

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H ---- C _______ C

/\

H

Stereochemical

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2 bond pairs and 0 lone pairs

linear

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4 bond pairs and 0 lone pairs

Tetrahedral

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3 bond pairs and 0 lone pairs

Trigonal planar

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3 bond pairs and 1 lone pairs

Trigonal pyramidal

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2 bond pairs and 2 lone pairs

angular

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1 bond pairs and 3 lone pairs

Linear tetrahedral

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In a ______, the negative (electron) charge is not distributed symmetrically among the atoms making up the molecule.

Polar molecule

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In a _______, electron distribution is symetrical

non-polar

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Polar molocules

HCL, CO, NH3, NF3, H2O, OCL, CHCL3, C2H5OH

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Non-Polar

CL2, N2, CO2, CH4

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If the atoms have the same electronegativivty →they attrect shared electrons equally = ________

Non polar covalent bond

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For a very large electronegativity diffrence, electrons may be transferred from one atom to another, thus cations and anions may form, and an _____________ will hold the compound together

Ionic bond

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If the atoms have diffrent electronegativities → the attraction for electrons is unequal = ____________

Polar covalent bonds

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The ____ the electronegativity diffreence, the _____ the bond

Greater, more polar

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NP

0.0 - 0.5

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Polar covalent

0.5 - 1.7

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Ionic

1.7 - 3.3

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The existence of a polar bond ______ necessarily mean that you have a polar molecule

not

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factors of polarity

shape of molecular and polarity of molecule

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in a ________ the bond dipoles will canclel each other out

nonpolar

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In a polar molecule, the bond dipoles ______ cancel each other out and will be nonzero molecule dipole, or an overal resilant vetctor

will not

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_______ compounds are solube in polar solvents

Polar

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_______ compunds are soluble in non-polar solvents

non-polar

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____molecular forces = forces attraction and repulsion between molecules

Inter

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____molecular forces = forces attraction within a molecule

Intra

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when molecules exert weak attractive forces on each other. Intermolecular forces vary over a mcuh wider range and are considerably weaker than the covalent bonds inside a molecule.

Van der waals forces

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In Van der waals forces experimental evidence: take _______ to boil water that it does to decompose water

Less energy

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In Van der waals forces, intermolecular forces are responisble for what we _______ about molecular substance

physically observe

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_______ forces appear to control the physical behaviour of molecular substances

Intermolecular

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The atrraction between dipoles is called _____

Dipole-dipole force

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dipole-dipole are amoung the _______ intermolecular

weakest

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Dipole-Dipole force exists only in ____ molecules

Polar

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Fritz london suggested that Van der waals forces was actually two forces

dipole-dipole, london force

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Is due to any electron movement within the molecule

momentary dipole

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Lond force is between ____ molecules

All

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As the number of electrons in the molecule _______, the boiling point increases

increase

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more electrons =

greater london force

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Isoelectronic

molecules with the same number of electrons

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if both are Isoelectronic what do you do?

Use dipole-dipole force

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  • between mols

  • weak

  • attration over greater distance

  • explains physical changes

Intermolecular

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  • Within mol

  • strong

  • attraction over smaller distance

  • explain chemical changes

Intramolecular

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a hydrogen nucleus is shared between pairs of electrons on adjacent molecules

Hydrogen bond

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For hydrogen bonding to occur, 2 this must be simultaneously true about the molecule structure.

  • Hydrogen must be covalently bonded to another very electronegative atom

  • there must be at least one lone pair on the atom bonded to the electrons

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Only three possible structures show hydrogen bonding

HF, -OH, -NH

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H bondingis not really a “bond” like a covalent bond, but rather an attraction _______ molecules

between

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