chem quiz 3

group 1 elements

alkali metals

group 2 elements

alkaline earth metals

group 17 elements

halogens (salt formers)

group 18 elements

noble gases

transition metals

3-12 groups

ductile

ability to be stretched into a thin wire (often metal)

malleable

able to be hammered without breaking (often metal) due to the metals’ valence electrons being able to slide past each other when force is applied

ionic bonds

between a nonmetal and a metal which attracts to each other due to cation and anion w/ diff. charges

ionic crystalline structure

strong and in a checkerboard pattern to maximize the attraction between positive and negative

anion type

nonmetals

cation type

metals

ionic compounds’ melting/boiling points

held together by strong electrostatic forces of attraction between positively and negatively charged ions

ionic solids’ electric conductivity

solids do not conduct electricity because ions are held in a rigid lattice and aren’t free to move

ionic solids’ electric conductivity IN WATER

are able to conduct because the water separates the ions and makes the ions free to move

ionic compounds when force breaks it

very brittle because their rigid crystal lattice structure shatter when the bonds break apart

covalent bonds

between two NONMETALS  and unable to be conductors because the electrons that they share aren’t free to move through the substance to conduct electricity

metallic bonds

electrostatic attraction between positively charged metal ions and delocalized MOBILE electrons shared among them which CONDUCTS electricity

strength of metallic bonds, ionic, and covalent in order

metallic>ionic>covalent (stronger bond=high boiling/melting points)

electronegativity

ability to attract electrons in the FIRST PLACE

electron affinity

energy released AFTER electrons attracted

electronegativity in groups

electronegativity decreases from top to bottom because the farther you are from the nucleus, the less attraction of electrons from the nucleus

nonpolar bonds

equal pull from both sides, electronegativity difference is .4 or less

polar covalent bonds

difference in electronegaitivity is .5 or greater, the one with the greater electronegativity is partially negative and vice versa

lone pairs

valence electron PAIRS that aren’t being shared in a bond

intermolecular forces

forces of attraction between different molecules

intramolecular forces

forces of attraction within the molecules

SNAP

symmetric-nonpolar symmetric-polar

London Dispersion force (LDF)

larger the molecule the stronger the force

hydrogen bond

strong intermolecular force that involves hydrogen directly bonded to F, O, or N. MORE HYDROGEN BONDS = STRONGER THAN LDF AND HYDROGEN.

dipole-dipole forces

forces of attraction between polar molecules

order of strength of bonds between LDF, ionic, and hydrogen

ionic>hydrogen»LDF

polar covalent and nonpolar compounds

polar covalent compunds are stronger due to the electrostatic attraction between partial charges

rules for naming IONIC compounds

1. name the cation

2. anion second followed by “ide”

rules for naming COVALENT compounds

1. first element keeps its name. FIRST ELEMENT GETS A PREFIX IF HAS SUBSCRIPT

2. second element gets “ide” and ALWAYS GETS A PREFIX 

prefixes for 1, 2, 3, 4, 5.

mono, di, tri, tetra, penta

rules for putting roman numerals in ionic compounds

1. find the ion charge of the second element and multiply it by the subscript of THE SECOND ELEMENT

2. divide that by the subscript on the first element and make it positive