Chapter 4 - Chemical Bonding

________ vibrate slightly, causing stretching and building that can cause the absorption of infrared radiation.

________ is especially good at trapping heat because it absorbs infrared radiation because of the unequal sharing of electrons within its bonds.

________: an atoms tendency to attract electrons toward itself in a chemical bond.

________: spreading out of electron density over multiple atoms, reducing the potential energy of electrons, therefore lowering the energy of the molecule (resonance stabilization)

________ symbols: depict an atoms bonding capacity- the number of bonds an atom typically forms to complete its octet.

Expanded Octet: nonmetals in ________ and below, such as P, S, Xe, etc.

________: different molecular forms of the same element, with different physical and chemical properties.

a pair of opposite charges separated by a distance; arrow points towards the more negative, electron- rich end of the bond

________: two- dimensional representation showing how atoms connect.

________: compounds containing unpaired valence electrons, tend to be very reactive to try to acquire or share an electron.

Add prefix hydro- to the name of the ________ in the formula.

________ is nitrous acid, HNO3 is nitric acid.

________ with the most oxygen has prefix per- and suffix- ate; ________ with fewest oxygens has prefix hypo- and suffix- ite.

________: name of parent element ending in- ide.

________ is sulfur dioxide.

________ is sodium chloride.

________: an unreal charge that assigns electrons to atoms within the molecule.

________ is an "average "of the two structures.

Consists of the ________ surrounded by dots on all four sides representing the valence electrons; all four sides must have one dot before electrons can be paired.

________: two atoms share one pair of electrons.

________: two atoms share three pairs of electrons.

________ is 0 on each element, but if impossible, most negative charge should be on the most electronegative element with formal charges as close to zero as possible.

________= (number of valence electrons)- (number of electrons in lone pairs- number of bonds)

electrostatic attractions between ions of opposite charge

energy released when free, gas-phase ions combine to form one mole of a crystalline solid

ordered 3-D array of particles

distance between two nuclei in the bond

amount of energy required to break one mole of bond into two moles of the free atom

unequal sharing of electrons between atoms; 2.0> Δχ> 0.4

represent the partial electrical charges

complete transfer of electrons; Δχ> 2.0

even distribution of charge, equal sharing of electrons; Δχ> 0.4

an atoms tendency to attract electrons toward itself in a chemical bond

name of parent element

name of parent element ending in -ide

all atoms except the very smallest (ex

two-dimensional representation showing how atoms connect

two atoms share one pair of electrons

two atoms share two pairs of electrons

two atoms share three pairs of electrons

pair of electrons that is not shared

different molecular forms of the same element, with different physical and chemical properties

2+ Lewis structures with same atomic arrangement but different arrangements of bonding electrons and lone pairs

spreading out of electron density over multiple atoms, reducing the potential energy of electrons, therefore lowering the energy of the molecule (resonance stabilization)

distance between the nuclei of two bonded atoms; depends on atomic identity and number of bonds formed

number of pairs of electrons atoms share

energy need to break one mole of bonds in the gas phase, always a positive quantity because breaking bonds requires energy; increases as bond order increases

an unreal charge that assigns electrons to atoms within the molecule

Be, B and Al

compounds containing unpaired valence electrons, tend to be very reactive to try to acquire or share an electron

nonmetals in third row and below, such as P, S, Xe, etc

infrared inactive

infrared active

infrared active