question

bonding lowers the

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potential energy between positive and negative

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Atomic Size -

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related to the distance between atoms in a sample of the element

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Transition Metals:

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the trend in size changes slightly since electron/electron repulsions counteract the decrease in size as we go across a period

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Ionization Energy -

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The energy required to remove an electron from an atom in the gas phase

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As atomic radius decreases, the ionization energy _____

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increases

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Electron Affinity -

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The energy change for a process in which an electron is acquired by the atom in the gas phase or “how bad an atom wants an electron.”

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Isoelectronic Ions:

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Ions that have the same number of electrons (but different number of protons). N-3, O-2, F-, Na+,and Mg+2

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Chemical Bond:

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When a chemical reaction occurs between two atoms, their valence electrons are reorganized so that a net attractive force occurs between atoms.

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Ionic bond:

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forms when one of more valence electrons is transferred from one atom to another. Produces a positive and negative ion. The “bond” is the attraction between the ions

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Covalent bond: forms by

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the sharing of valence electrons between atoms.

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Metal with nonmetal bonding –

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electron transfer and ionic bonding

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Covalent bonding –

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occurs most commonly between non mental atoms

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Metal with metal bonding –

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electron pooling and metallic bonding

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Metallic bonding –

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metal atoms sharing valence electrons but not by covalent bonding

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Octet rule –

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when atoms bind, they lose, gain, or share electrons to attain a filled outer level of eight electrons or two for H and Li

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The lattice energy

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the enthalpy change that occurs when 1 mol of ionic solid separates into gaseous ions

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Ionic solids exist only because

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the lattice energy exceeds the energy required for the electron transfer

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Formation of a covalent bond always results in

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a greater electron density between the nuclei

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Bond order –

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the number of electron pairs being shared by a given pair of atoms

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Single bond –

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the most common band and consists of one bonding pair of electrons

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Double bond –

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consists of two bonding pairs of electrons, four electrons shared between two atoms so the bond order is 2

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Bond energy –

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the energy needed to overcome this attraction and is defined as the standard enthalpy change for breaking the bond in 1 mol of gaseous molecules

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Bond length –

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the distance between the nuclei of the two bonded atoms

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Bond order to directly related to _____and inversely related to ______

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bond energy; bond length

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Most covalent substances have low electrical conductivity because

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their electrons are localized and ions are absent

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Electronegativity –

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the relative ability of a bonded atom to attract shared electrons

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An important use for electronegativity is

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determining an atom’s oxidation number

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When atoms of different electro negativities form a bond, the bonding pair is shared ____

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unequally

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Polar covalent bond –

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unequal distribution of electron density

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Electronegativity difference -

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the difference between the electronegativity values of the bonded atoms

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Electronegativity difference is directly related to a bond’s _____

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polarity

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As the ?EN decreases, the bond becomes more ____

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covalent

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Bond Dissociation Enthalpy:

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the enthalpy change for breaking a bond in a molecule with the reactants and products in the gas phase

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Polar Bond:

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When the bond between two atoms has a positive and negative end or pole.

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Hydrogen atoms from ____ bonds

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one

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Carbon atoms from _____ bonds

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four

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Nitrogen atoms form _____ bonds

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three

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Oxygen atoms form ______ bonds

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four

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Fluorine is always a ______

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surrounding atom

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Resonance structures –

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have the same relative placement of atoms but different locations of bonding and lone pairs

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Resonance hybrid –

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average of the resonance forms

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Partial bonding in resonance hybrid, often leads to ______

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fractional bond orders

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Formal charge –

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change an atom would have if the bonding electrons were shared equally

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Electron deficient –

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have fewer than eight electrons around the central nucleus

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Free radicals –

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species that contain a lone (unpaired) electron, which makes them paramagnetic and extremely reactive

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Expanded valence shells occur only with _______ because they have d orbital available

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nonmetals form period 3 or higher

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VESPR Theory –

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to minimize repulsions, each group of valence electrons around a central atom is located as far as possible from the others

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Molecular shape –

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three dimensional arrangement of nuclei joined by the bonding groups

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The electron group arrangement is defined by

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the bonding and nonbonding electron group

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The Molecular shape is defined by

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the relative positions of the nuclei, which are connected by the bonding groups only

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Bond angle –

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angle formed by the nuclei of the two surrounding atoms with the nucleus of the central atom at the vortex

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Linear shape –

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AX2 108o

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Trigonal Planar–

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AX3 120o

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Tetrahedral –

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AX4 109.5o

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Trigonal Bipyramidal –

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AX5 90o & 120o

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Octahedral –

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AX6 90o

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Lewis electron dot symbols: developed by

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Gilbert Newton Lewis

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Bond pair:

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The e- involved in the covalent bond.

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Lone pair:

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The e- not involved in bonding also called nonbonding e-.

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Octet Rule:

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The tendency of molecules and polyatomic ions to have structures in which eight e- surround each atom

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Valence shell electron-pair repulsion is a method for

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predicting the shapes of covalent molecules and ions.

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Electron-pair geometry:

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the geometry taken up by ALL the valence e- pairs around a central atom

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Molecular geometry describes

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the arrangement in space of the central atom and the atoms directly attached to it.

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Valence Bond Theory created by

answer

Linus Pauling

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Bonding between the two atoms occurs when

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the e- clouds on the two atoms interpenetrate or overlap

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Orbital overlap increases the probability of

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finding bonding e- in this region of space.

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The idea that bonds are formed by overlap of atomic orbitals is the basis for

answer

valence bond theory.

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The covalent bond that arises from the overlap of the two s orbitals (1 from each H) is called

answer

a sigma bond.

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Liquids and solids resist

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compression

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Dipole-Dipole Attraction:

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when one polar molecule encounters another, the positive end of one is attracted to the negative of the other, and via versa.

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Hydrogen Bond:

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The strong attraction between an electronegative atom with a lone pair and the hydrogen atom of the N--H, O--H, or F--H bond.

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Dipole/Induced Dipole Forces:

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polar molecules can induce a dipole in a molecules that do not have a permanent dipole.

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As the water molecule approaches the O2 molecule a dipole is induced, this is referred to as _____

answer

polarization.

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The degree to which the e- cloud distorts is called ______

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polarizability.

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The larger the molar mass the greater the _____

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polarizability of the molecule.

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Dipole/Induced Dipole Forces are weaker than _____

answer

electrostatic or dipole/dipole interactions.

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Induced Dipole/Induced Dipole Forces are often referred to as _______

answer

London dispersion forces

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London forces arise between

answer

all molecules both polar and non-polar

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London dispersion forces are the only intermolecular forces that

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allow non-polar molecules to interact

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Vaporization:

answer

or evaporation is the process in which a substance in the liquid phase becomes a gas

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The standard molar enthalpy of vaporization, ?vapHo (kJ/mol):

answer

the energy required to vaporize a sample.

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Condensation:

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when a molecule loses efficient energy to reenter the liquid phase. (exothermic)

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Equilibrium Vapor Pressure:

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the pressure exerted by the vapor in equilibrium with the liquid phase.

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The tendency of its molecules to escape from the liquid phase and enter the vapor phase, referred to as _______

answer

volatility.

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Critical Point:

answer

when a specific temp and pressure are reached, the interface between the liquid and the vapor disappears.

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Critical Temperature:

answer

the temperature at which this phenomenon is observed, and the corresponding pressure, critical pressure

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Viscosity:

answer

the resistance of liquids to flow

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Surface Tension:

answer

the energy required to break through the surface or to disrupt a liquid drop and spread the material out as a film.

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