Chemical bond
like glue/the force that holds two atoms together. Can form by the attraction between positive ions and negative ions and the positive nucleus and negative electrons
Cations
a positively charged ion; most common are those produced by loss of valence electrons from metal atoms
Anion
a negatively charged ion; end in -ide; gained by neutral atom
Ionic bonding
the electrostatic forces that hold oppositely charged particles together; made of cations and anions; they are electrically neutral
Ionic Compounds
salts, compounds that contain ionic bonds; physical structures are unique, large number of +ions and -ions exist in a ratio determined by the number of electrons transferred from a metal atom to a non-metal atom; packed into a regular repeating pattern, balances forces of attraction and repulsion between ions;
Crystal lattice
a three-dimensional geometric arrangement of particles
Electrolytes
an ionic compound whose water solution conducts an electric current
Lattice energy
the energy required to separate 1 mol of the ions of an ionic compound (energy needed to break up electrolyte);the greater the charge of the ions the greater the lattice energy is; the smaller the size of the ion, the more lattice energy
Formula unit
Chemical formula that represents the simplest ratio of ions involved
Monatomic ion
a one-atom ion, such as Mg²⁺ or Br⁻
Oxidation number
the charge of a monatomic ion.
Polyatomic ions
ions made up of more than one atom that are bonded together that acts as a single unit with a net charge. (ex. Nitrate= NO₃⁻) End in -ite, -ate
Oxyanions
a polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms.
Ionic crystal
hard ridged brittle solids, due to strong attractive forces holding ions in place at room temp (Mohs scale); crystal breaks apart because applied force repositions the like-charged ions next to each other
properties of ionic compound
solid, hard, brittle, high melting/boiling points, can conduct eletricity when melted or desolved in water, well-designed crystals at room temp
valence electrons
the electrons in the highest occupied energy level of the elements atom, farthest from the nucleus. The number of valence electrons determines the chemical properties of the element; they are grouped together on the periodic table (ex. group 1 have 1 valence electron, group 4 have 4 valence el); they are the only electrons used in a chemical bond; dots in dot structure
Dot structure
Lewis, how many electrons in the valence shell (most outer energy level)
formula unit/ ratio
lowest whole-number ratio of ions in an ionic compound. NaCL = 1:1
pseudo-noble gas configuration
electron configurations other than the octet rule that give some stability, for example groups 11-14 may have full s, p, d sublevels
-ide
ending of an anion
properties of ionic compounds
strong attraction between oppositely charged ions means:high melting & boiling pointsionic crystals are very hard but brittleconduct electricity when dissolved in solution or melted (ELECTROLYTES)
Electrolyte
substance that forms ion when it is dissolved in water, capable of conducting an electrical current
What is the compound of Al and S
Al₂S₃
Name MgO
Magnesium Oxide
metallic bond
The electrostatic attraction between cations and the negatively charged sea of electrons.
delocalized electrons
these electrons do not orbit any particular atom, but constantly move among different atoms-this creates a "sea" of electrons throughout the metal
electron sea model
simplest picture model. pictures a regular array of metal atoms in a "sea" of valence electrons that are shared among the atoms in a nondirectional way
properties of metallic bonds
mealable, ductile
aluminum
will always have a +3
silver
will always be +1
zinc
will always be +2
Acetate ion
C₂H₃O₂⁻
Carbonate ion
CO₃⁻²
Sulfate ion
SO₄⁻²
Phosphate ion
PO₄⁻³
Nitrate
NO₃⁻
amonium ion
NH₄⁺
Hydroxide
OH⁻
Cyanide ion
CN⁻
____ alloys are formed when some atoms in the original metallic solid are replaced by other metals of similar atomic structure.
substitutional
____ alloys are formed when small holes in a metallic crystal are filled with smaller atoms.
interstitial
An ____ is a mixture of elements that has metallic properties. (mixture not compound which allows for different strengths)
alloy
The properties of alloys ____ from the elements they contain
differ
____ electrons around cations make metals _____ conductors of electricity and heat.
Mobile, good
As the number of delocalized electrons _____, so does hardness and strength.
increases
Metals are ____ because they can be hammered into sheets.
malleable
Metals are _____ because they can be drawn into wires.
ductile
Boiling points are much _____ extreme than melting points because of the energy required to _____ atoms from the groups of cations and electrons.
more, separate
A ______ is the attraction of a metallic cation for delocalized electrons.
metallic bond
Within the crowded lattice, the outer energy levels of metal atoms _____.
overlap
The electron sea model proposes that all ______________________ contribute their valence electrons to form a "sea" of electrons. The electrons are free to move around and are referred to as _____ electrons, forming a metallic cation.
metal atoms in a metallic solid delocalized
Metals are not ionic but ___________________________.
share several properties with ionic compounds.
Metals also form lattices in the _, where 8 to 12 other atoms ___________________.
solid state, closely surround each metal atom.
Chemical _____ is a systematic way of naming compounds.
nomenclature
An _______ is a polyatomic ion composed of an element (usually a non-metal), bonded to _________.
oxyanion, bonded to one or more oxygen atoms.