Unit 3 Key Terms/Concepts Flashcards by Brashe Webster

What are the 4 ways to represent electron configuration?

Full configuration
Short hand/core/condensed
Lewis/Electron-Dot symbols

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To find the number of valence electrons in an element, you must know the _____, because they are equivalent (except for Helium)

The group number on the periodic table

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what is the maximum number of dots per side in a Lewis configuration

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Octet rule

atoms tend to gain, lose, or share
electrons in order to obtain an octet in their valence
shells due to the stability of the ns^2p^6 configuration.
(2+6 = 8; octet = set of 8)

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elements that follow the duet rule (not the octet rule)

H, He, Li, and Be

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Nonmetals tend to ___ an electron to reach an octet

gain

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metals ___ their valence electrons to become cations

lose

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covalent bonds

a pair of electrons shared between two atoms.

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binary covalent compounds.

Compounds containing two different nonmetals that

share valence electrons

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a compound is ionic if

the first element is a metal or it starts with the polyatomic ion NH4+ (ammonium ion).

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Potassium oxide

K2O

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a binary compound is covalent if

the first element in the formula or the name is a

nonmetal.

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N2O

dinitrogen monoxide

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acid

a substance that releases H+ ions (or protons or hydronium ions) in water solutions.

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Most acid formulas start with

H (Hydrogen)

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monoprotic acids

can produce only one H+ (or proton or hydronium ion) in water

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polyprotic acids

Acids that can produce two or more H+’s in water

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Binary acids contain

H and one other element (Not Oxygen)

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Binary acids are named according to what pattern

hydro + part or all of element name + ic acid

Ex: HCl hydrochloric acid

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Oxyacids (oxoacids) contain

O (Oxygen)

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The general formula for oxyacids is

General formula = HnXOm (X is the “central

atom”)

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Oxyacids containing -ate ions end with___

-ic acid

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Polyatomic names determine the

oxyacid name

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Oxyacids containing -ite ions end with

-ous acid

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water formula

H2O

Hydrogen Peroxide

H2O2

Methane

CH4

Ammonia

NH3

C2H5OH

drinking alcohol, ethyl alcohol or ethanol

HC2H3O2 or CH3COOH

vinegar/acetic acid (5%)

C3H7OH

rubbing alcohol/ isopropyl alcohol/or 2-propanol

nail polish remover/ acetone

C3H6O

one shared pair of electrons is .

a single covalent bond

Double bond

two shared pairs of electrons

Lone pair or Non-bonding electron pair

A lone pair does not participate in bonding (it is not shared).

Give correctly spelled name for the following compound: | CO

Carbon Monoxide

Give correctly spelled name for the following compound: | CO2

Carbon Dioxide

Give correctly spelled name for the following compound: | PCl5

phosphorus pentachloride

Give correctly spelled name for the following compound: | P4O10

tetraphosphorus decoxide

dinitrogen pentoxide

N2O5

hydrogen sulfide

H2S(g)

Give correctly spelled name for the following compound: | HCl(aq)

hydrochloric acid

Give correctly spelled name for the following compound: | hydroselenic acid

H2Se(aq)

Give correctly spelled name for the following compound: | H2SO3(aq)

sulfurous acid

Give correctly spelled name for the following compound: | HClO(aq)

hypochlorous acid

sulfur hexafluoride

SF6

xenon tetrafluoride

XeF4

carbon disulfide

CS2

sulfur trioxide

SO3

dinitrogen tetroxide

N2O4

silicon dioxide

SiO2

dichlorine heptoxide

Cl2O7

sulfur dichloride

SCl2

hydrobromic acid

HBr(aq)

hydrosulfuric acid

H2S(aq)

nitric acid

HNO3(aq)

phosphoric acid

H3PO4(aq)

chlorous acid

HClO2(aq)

periodic acid

HIO4(aq)

Identify the electron domain geometries of the central atoms in the compounds and ions: H2O

tetrahedral (2 bonds, two lone pairs)

Identify the electron domain geometries of the central atoms in the compounds and ions: H2SO3

tetrahedral (3 bonding domains, 1 lone pair)

Identify the electron domain geometries of the central atoms in the compounds and ions: CN-

linear around C (triple bond counts as one e- domain, 1 lone pair)

Identify the electron domain geometries of the central atoms in the compounds and ions: ClF3

trigonal bipyramidal (3 bonds, 2 lone pairs)

Identify the electron domain geometries of the central atoms in the compounds and ions: XeF4

octahedral (4 bonds, 2 lone pairs)

Identify the electron domain geometries of the central atoms in the compounds and ions: HNO3

trigonal planar for the central N (3 bonding domains; double bond counts as one)

With a trigonal planar electron-domain geometry, molecular shapes may be

either trigonal planar or bent (nonlinear, V-shaped).

Molecules with a tetrahedral electron-domain geometry can havewhyat types of molecular geometries?

tetrahedral, trigonal pyramidal, or bent shapes.

True or false: Bonding Electron pairs occupy more space than nonbonding pairs.

False

True or false: Lone pairs can cause some bond angles to change.

True

If a central atom has 5 electron domains, four different molecular shapes are possible.

Trigonal Bipyramidal, See Saw, T-Shaped, and Linear (3 lone pairs)

Four molecular shapes are possible if a central atom has six electron domains. (6 electron domains)

Octahedral, Square Pyramidal, Square planar, T-Shaped

How do you find hte molecular shape of a molecule when given a formula

1) Determine the Lewis structure. 2) Figure out the electron domain geometry. 3) Determine the molecular shape. (Be able to draw it using wedge notation.)

Bond angles and the actual shape of the molecule are determined by

the electron domain geometries around the central atoms.

True or False: Lewis structures show actual geometries of molecules.

False

If atoms of two different elements are bonded, electron sharing is often

unequal

Partial charge (S)

a charge that is not a full positive or full negative charge.

Electronegativity

a measure of the tendency of an atom to attract the electron density of a bond.

Electronegativity follows the same trend as

ionization energy and electron affinity

polar covalent bond

A covalent bond between atoms in which electron sharing is significantly unequal

The extent to which a covalent bond is polar is determined by the difference in

electronegativities (high minus low)

Bond dipole

a shift in the electron density in a bond due to differences in electronegativities between two bonded atoms. A polar covalent bond has a bond dipole.

--|------>

The symbol for a bond dipole

The bigger the difference in the electronegativies of two bonded atoms, the more _____ the bond is

Polar

A bond between two atoms of the same element will be

nonpolar

With an electronegativity difference of 1.7, bonds are said to have

50% ionic character.

> 1.7 electronegativity difference

ionic bond (usually)

> 0.35 to 1.7 electronegativity difference

polar covalent bond

0 to 0.35 electronegativity difference

nonpolar bond (usually)

Polar molecule

a molecule with a net dipole moment. A molecule with a partially positive side and a partially negative side.

Nonpolar molecule

a molecule with a net dipole moment of zero. A molecule that does not have opposite partial charges on different ends of the molecule.

Dipole moment

the sum of the effects of the bond dipoles (from polar covalent bonds), taking the geometry of the molecule into account

Carbon dioxide contains polar bonds but the bond dipoles cancel each other. The molecule is _____

nonpolar

A water molecule is _____because the bond dipoles add together.

polar

If the structure is balanced, the molecule is

nonpolar (no pull to one side more than the other).

If something about the structure is not balanced, the molecule is

polar - electron density will be pulled to one side more than the other.

To write a formula for a covalent compound

list the element symbols in the same order as they appear in the name. • write the numbers indicated by the prefixes as subscripts after the element symbols.

Unit 3 Key Terms/Concepts Flashcards

(96 cards)