Chemistry test 3

polyatomic ion

A charged group of covalently bonded atoms

ionic bonding

Chemical bonding that results from the electrical attraction between cations and anions

polar covalent bond

Covalent bond in which the bonded atoms have an unequal attraction for shared electrons

Lewis structures

Formulas in which atomic symbols represent nuclei and inner-shell electrons

Halogens

Group 17

transition metals

Group 3 through 12

Periods

Horizontal rows on the periodic table

4 (s, p, d, f)

How many sub levels are in the 4th energy level?

Then the name must be changed

If the element has a negative charge

alkaline earth metals

Name of group 2 elements

Formula unit

Simplest collection of atoms from which an ionic compound's formula can be written

Sr

Sr Which element has the following configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2

Aufbau principle

States that electrons will enter the lowest, or first open energy level first

London dispersion forces

The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles

P block

What block is Ar in

F block

What block is Ce in?

D block

What block is Hg in?

S block

What block is Na in?

S block

What block is helium in?

Charge

What does the Roman numeral in a name mean

Place the first 10 electrons

What does this notation mean: [Ne]

Sulfur

What element has the following configuration: 1s^2 2s^2 2p^6 3s^2 3p^4

1s2 2s2 2p6 3s2 3p6 3d6 4s2

What is the FULL electron configuration for Iron?

[Kr] 5s2

What is the abbreviated electorn configuration Strontium?

Li2S

What is the correct formula for Lithium Sulfide?

4f (because it is in the f block)

What is the last entry in the configuration for Samaritan

Ide

What is the negative ending

4s

What is the next step in the configuration pattern: 1s 2s 2p 3s 3p

4

What is the valence shell on an atom of Potassium

Hund's Rule

What rule sates that electrons will sit together only when they need to

He left spaces for undiscovered electrons

What was so important about mendelelv's table vs the other tables at the time

Sr

Which of the following is the smallest element

S and p

Which of the following shows the correct sublevels for the 2nd principal energy level

1s2 2s2 2p6 3s2 3p4

Write out the full electron configuration for silicon-28

Superscript

Written above and smaller then the atom: the charge Ma^+1

Subscript

Written in smaller and below the symbol: The number of atoms Na(tiny)2

Molecular compound

a chemical compound whose simplest units are molecules

Single bond

a covalent bond in which one pair of electrons is shared between two atoms

nonpolar covalent bond

a covalent bond in which the electrons are shared equally by the two atoms

Chemical bond

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

Molecule

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

electron-dot notation

an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element's symbol

Ionic compound

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

Dipole

created by equal but opposite charges that are separated by a short distance

Multiple bonds

double and triple bonds

1s2 2s2 2p6 3s2 3p6 4s2 3d8

full electron configuration for nickel full electron configuration for nickel

Structural formulas

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

Chemical formula

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

Hybridization

mixing of two or more atomic orbitals of similar energes on the same atom to produce new hybrid atomic orbital equal energies

Hybrid orbital

orbitals of equal energy produced by the combination of two or more orbitals on the same atom

Resonance

refers to bonding in molecules or ions that cannot be correctly represented by a single Lewis structure

Covalent bonding

results from the sharing of electron pairs between two atoms

Molecular formula

shows the types and numbers of atoms combined in a single molecule of a molecular compound

VSEPR theory

states that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible

Ductility

the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire

Malleability

the ability of a substance to be hammered or beaten into thin sheets

metallic bonding

the chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons

Lattice energy

the energy released when one mole of an ionic crystalline compound is formed from gaseous ions

Bond energy

the energy required to break a chemical bond and form neutral isolated atoms

Hydrogen bonding

the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule

Polar

uneven distribution of charge