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