• Shuffle
    Toggle On
    Toggle Off
  • Alphabetize
    Toggle On
    Toggle Off
  • Front First
    Toggle On
    Toggle Off
  • Both Sides
    Toggle On
    Toggle Off
  • Read
    Toggle On
    Toggle Off
Reading...
Front

Card Range To Study

through

image

Play button

image

Play button

image

Progress

1/47

Click to flip

Use LEFT and RIGHT arrow keys to navigate between flashcards;

Use UP and DOWN arrow keys to flip the card;

H to show hint;

A reads text to speech;

47 Cards in this Set

  • Front
  • Back
Atomic Structure
Protons Neutrons, Electrons
• 3 subatomic particles make up all atoms: electrically positive protons, electrically neutral neutrons, and electrically negative electrons.
• The more massive protons and neutrons are contained with in the nucleus of an atoms as well as most of the atoms mass and all the positive charge.
• Electrons which have a much smaller mass surround the nucleus and occupy much of the volume
• Chemical properties depend largely on the electrons of the atoms involved
Atomic Number
o All atoms of a given mass have the same number of protons in the nucleus
o The symbol Z is given to this number and is the atomic number
o Integer number at the top of the box in the periodic table is the atomic number
Atomic Weight/Mass
o Substances produced had constant composition and so the relative mass could be defined
o Carbons Mass-12 because it has 6 protons and 6 neutrons
o Oxygen has 8 protons and 8 neutrons and has 1.3329 times the mass of carbon there for is has a mass of 15.9949
Atomic mass units (u)
used to express mass
• One atomic mass unit, 1u, is one 12th the mass of an atom of carbon with six protons and six neutrons
Mass Number
o Protons and neutrons have masses very close to 1u
o Mass of an electron 1/2000 of a u
o Approximate mass of an atom can be estimated if the number of neutrons and protons is known an is called the mass number
Isotopes
o Most elements consist of atoms that have several different mass numbers
o Atoms with the same atomic number but different mass numbers are called isotopes
o All atoms of an element have the same number of protons
o To have different mass isotopes must have different numbers of neutrons
Molecular form
• F2-9
• Diatomic molecules: e.g. H2, N2, O2, halogens
• Triatomic molecules: e.g. O3
• Allotropes- different chemical forms of the same element
• Dioxygen or oxygen O2
• Trioxygen or ozone O3
Allotropes of carbon
• Diamond
o Has a diamond form
• Graphite
o Conduct electricity
o Hexagonal shaped
o 3 carbons connected
molecular compounds- consist of molecules
• F2-13
• Ethanol C2H6O molecular formula
o Have 2 carbon atoms per molecule of C2H6
Ionic Compounds
• Compose of ions
• Ions charged particles that result from the gain or loss of electrons
• Cations- positively charged
• Anions- negatively charged
Monatomic
o Single atom with a charge
o Fixed charged ions
o Elements form 1 charge only
o Li+
Polyatomic ions
o Groups of atoms with a charge
o Soy2- (like a molecule with a charge
o T2-y
o Most are anions
Charges of metals
tend to be electropositive they tend to loose electrons to become cations
Charge on non-metals
to be electronegative, they tend to gain electrons to be come anions
o F is the most electronegative element O is the second
Variable charged cations
• Include most transition elements
• Some others such as Sn, Pb
Fixed charged cations
o For main group elements the charge equals the groups
• 1A- H+, C+,
• 2A- Be2+, Mg2+
• 3A- Al3+, Ga3+
charge of transition elements
• Ag+, Zn2+, Cd2+
dual nature if hydrogen
o Hydrogen can lose an electron to become H+(a proton)
o Gain an electron and become H- like He
o It can also form molecules single hydrogen atom
• They share electrons
• Covalent bound
Ionic Compounds
o Look at the compound and know if its ionic compound
o Usually contains a metal and a non metal
o Exception is if it contains ammonium
Naming Ionic Compounds
• Cation first then the anion
• Ions name ends with the word ions
• Ex-Na+ sodium ion, Cl- chloride ion
• Cation name then anion name lose ion
• Ex- NaCl is sodium chloride
Cation Names
• Fixed charged monatomic ions
• Elements name followed by the word ions
• Ex-H+ hydrogen ion, Na+ sodium ions, Mg+2 magnesium ion
Variable charge monatomic ions name
• Element name + charge using roman numerals (in parentheses)+word “ion”
• Cu+ copper (I) ion, Cu2+ copper (II) ion, Fe2+ iron (II) ion, Fe3+ iron (III) ion stock system
Naming Monatomic anions
o Element root name + the suffix “ide”
o Ex-Cl- chloride ion
Naming Polyatomic anions
o CN- cyanide ion
o C2H3O3 or CH3CO2- acetate ions
Naming Oxoanions
o ClO- hypochlorite ion, ClO2 chlorite ion, ClO3- chlorate ion, ClO4- perchlorate ion
o SO32-, SO42-
o PO43- phosphate ion + H+= HPO42- hydrogren phosphate ion, H2PO4- dihydrogen ion, H3PO4
Binary molecular compounds
o 2 elements
o non-metals only
o pre-fix 1 + the first element name=first word, pre-fix + element root + “ide”=2nd word
o N2O5 Dinitrogen pentaoxide (pentoxide)
o CO-carbon monoxide
o SiCl4-Silicon tetrachloride
o N2O3- dinitrogen trioxide
o SF6 monsulfur hexafluoride
Molecular compounds that contain Hydrogen
o H2S dihydrogen monosulfide full systematic, most commonly know as hydrogen sulfide
o Since hydrogen is the simplest element it combines with other elements in a predictable way the naming of he compound is sometimes simplified almost treated like an ionic compound
o Ex-2 Na+ + S2- = Na2S sodium sulfide ionic compound
o Ex- 2H+ + S2- = H2S hydrogen sulfide
o Ex- H2O- dihydrogen monoxide sometimes hydrogen oxide
o Ex- H2O2- dihydrogen dioxide common name is hydrogen peroxide
o HCl (g)- common name is hydrogen chloride
o HCL- (aq)- hydrochloric acid
1) Coulombs law
a) 1(u)
b) Electric charge
c) force if attraction between ions of opposite charge increase as the magnitude of the charges increase and decreases as the distance between the ions increase
2) Melting pt
a) The stronger the forces between particles the high temp is needed
Ammonium ion
NH4+
cation
Carbonate ion
C2H3O2- or CH3CO2-
Chlorate ion
CIO3-2
Chlorite ion
CIO2-
Chromate ion
CrO4-2
Cyanide ion
CN-
Dichromate ion
Cr2O7-2
Dihydrogen phosphate ion
H2PO-4
Hydrogen Carbonate
HCO3-
Hydrogen Phosphate ion
HPO4-2
Hydrogen Sulfate
HSO4-
Hydroxide ion
OH-
Hypochlorite ion
ClO-
Nitrate ion
NO3-
Nitrite ion
NO2-
Perchlorate ion
CIO-
Phosphate ion
PO4-
Sulfate ion
SO4-2
Sulfite ion
SOs-2