Chem Unit 5 Flashcards
Ions
Atoms that lose or gain electrons
The Ocet Rule
Atoms will gain or lose atoms in order to completely fill up the outermost shell with 8 electrons
Ionic bond basic
At least one metal and one nonmetal, electrons are transferred from metal to nonmetal
Covalent bond basic
Only non metals, electrons are shared between no metals
Metallic bond basic
Only metals, electrons are delocalized
Type of structure of bonds
Ionic- crystal lattice
Covalent- true molecules
Metallic- “electron sea” or crystal structure
Phase at room temp and melting point
Ionic- solid at room temp, high melting point
Covalent- liquid or gas at room temp, low melting point
Metallic- solid at room temp, very high melting point
Solubility and electrical conductive kitty
Ionic- soluble, conducts electricity but only when dissolved in water or in liquid form
Covalent- usually not double, not a conductor
Metallic- not soluble, conducts electricity
Covalent bond
An electrostatic attraction of electrons to two different nuclei that holds the nuclei together
Purpose of bonds between atoms
To increase stability of the neutral atom
To decrease potential energy (the bond energy)
Naming monatomic ion
for a cation leave the name as is
For anions drop the end and add -
ide
(Oxide)
Naming binary ionic compounds
Metal/Cation goes first, nonmetal/anion goes last
When determining formula from compound name, add enough molecules so positive charge equals negative charge
NaCl)
Naming transition metals
Charge of ion must be indicated in name of compound
Polyatomic ions
Ions made up of covalent my bonded atoms that have an overall charge, with special names
Ammonium
NH4+1
Hydroxide
OH-1
Carbonate
CO3-2
Chlorate
ClO3-1
Chlorite
ClO2-1
Cyanide
CN-1
Nitrate
NO3-1
Nitrite
NO2-1
Phosphate
PO4-3
Phosphite
PO3-3
Sulfate
SO4-2
Sulfite
SO3-2
Naming covalent compounds
Prefixes identify number of each element in the name
Prefixes
1-mono 2-di 3-tri 4-tetra 5-penta 6-hexa 7-hepta 8-octa 9-nona 10-deca
Saturated vs unsaturated hydrocarbons
Saturated is the there is the maximum number of hydrogen atoms connected to the available carbons, and unsaturated means there’s at least one double or triple bond
Alkanes
A hydrocarbon where there are only single covalent bonds between the carbon and hydrogen atoms
Alkenes
At least one double bond in the carbon-carbon bond
Alkynes
At least one or more triple covalent bond
Structures vs condensed formula
Structured shows position of every single atom, while condensed shows the bonds in groupings (CH3-CH2-CH3)
Line Angle Formula
Carbons and hydrogen atoms are removed. Bonds between carbons shown as a “zigzag” line, but all other atoms are shown
Prefixes for naming Alkanes
1-meth 2-eth 3-prop 4-but 5-pent 6-hex 7-hept 8-oct 9-non 10-dec
Structural isomers
Molecules that have the same molecular formulas but a different arrangement of atoms (different structural formulas)
Geometric isomers
Have atoms joined in the same order, but differ in the orientation of groups around a double bond
Cis configuration
The substituent groups are on the same side of the double bond
Trans configuration
The substituent groups are on opposite sides of the double bond
Lewis dot diagram
Write element symbol, then draw in number of valence electrons around it
