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87 Cards in this Set
- Front
- Back
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What Formulas are Ionic
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Metals and non Metals
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What Formulas are Molecular
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Non Metals Only
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What Formulas are Acidic
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Starts with an H and one or more non metal
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What is the Naming Scheme for Molecular Compounds
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Prefix.. first element.. prefix... second element.. add -ide to the end
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What does this Prefix Mono- Mean
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one
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What does this Prefix Di- Mean
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two
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What does this Prefix Tri- Mean
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three
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What does this Prefix Tetra- Mean
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four
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What does this Prefix Penta- Mean
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five
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What does this Prefix Hexa- Mean
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six
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What does this Prefix Hepta- Mean
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seven
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What does this Prefix Octa- Mean
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eight
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What is the Naming Scheme for Ionic Compounds
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name of cation (metal)... (charge of cation if it has more than one)... base name of anion plus -ide at the end
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What are the possible Cations of Fe
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2+ and 3+ (Iron) *
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What are the possible Cations of Cu
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1+ and 2+ (Copper) *
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What are the possible Cations of Zn
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2+ (Zinc) *
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What are the possible Cations of Ag
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1+ (Silver) *
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What is the Naming Scheme for Acidic Compounds
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No Oxygen- Hydro... base name of non metal plus -ic... "acid" (hydro ____ic acid) With Oxygen- Base name of Oxyanion and (ate -> ic , ite -> ous)... acid
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Name this Polyatomic Ion: PO4 -3
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phosphate
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Name this Polyatomic Ion: HPO4 -2
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hydrogen phosphate
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Name this Polyatomic Ion: H2PO4 -1
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dihydrogen phosphate
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Name this Polyatomic Ion: CO3 -2
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carbonate
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Name this Polyatomic Ion: HCO3 -1
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hydrogen carbonate or bicarbonate
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Name this Polyatomic Ion: ClO 1-
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hypochlorite
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Name this Polyatomic Ion: ClO2 -1
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chlorite
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Name this Polyatomic Ion: ClO3 -2
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chlorate
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Name this Polyatomic Ion: ClO4 -1
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perchlorate
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Name this Polyatomic Ion: C2H3O2 -1
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acetate
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Name this Polyatomic Ion: MnO4 -1
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permanganate
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Name this Polyatomic Ion: C2O4 -2
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oxalate
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Name this Polyatomic Ion: NH4 +1
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ammonium
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Name this Polyatomic Ion: NO2 -1
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nitrite
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Name this Polyatomic Ion: NO3 -1
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nitrate
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Name this Polyatomic Ion: SO3 -2
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sulfite
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Name this Polyatomic Ion: HSO3 -1
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hydrogen sulfite or bisulfite
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Name this Polyatomic Ion: SO4 -2
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sulfate
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Name this Polyatomic Ion: HSO4 -1
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hydrogen sulfate or bisulfate
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Name this Polyatomic Ion: OH -1
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hydroxide
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Name this Polyatomic Ion: CN -1
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cyanide
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Name this Polyatomic Ion: Cr2O7 -2
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dichromate
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Name this Polyatomic Ion: CrO4 -2
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chromate
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Name this Alkane C6H14
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Hexane
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Name this Alkane C7H16
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Heptane
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Name this Alkane C8H18
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Octane
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Name this Alkane C9H20
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Nonane
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Name this Alkane C10H22
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Decane
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Define Compound |
Substance of two or more atoms combined in a specific ratio |
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Define Empirical Formula |
The simplified molecular formula |
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Define Molecular Formula |
The actually ratio of atoms in the molecule |
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Define Allotrope |
It is a element of two different natural forms with different chemical formulas (carbon as graphite and diamonds) |
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Bonding is just a type of ___________ |
Modeling |
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What is the electronegativity trend |
it goes higher as you go up and to the left (except the nobel gases) |
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What number of one mole |
6.022 x 10^23 |
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triple bond is _____ than double bonds |
shorter and stronger |
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What is a lattice |
it is the structure of an ionic compound |
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what is lattice energy and how to find it |
lattice energy is the amount of energy required to turn a mole of ionic solid to a gas. it depends on the charge and the distance between them. |
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what is the trend for radii of atomic molecules |
is gets bigger as you move down and to the left |
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what is the difference between ionic and covalent bonding |
ionic bonding is when a non metal takes an electron from a metal, creating two ions with opposite charges and making it so that attract |
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what are the homonuclear diatomic molecules |
it makes a seven shape adding Hydrogen (h2, N2, O2, F2, Cl2, Br2, I2) |
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what is heteronuclear diatomic molecules |
they are covalent molecules with two different atoms |
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How do you draw dot structures? |
1. find the total number of valence electrons in the molecule (adding one for each positive and subtracting one for each negative) 2. decide the central atom (least electronegative except hydrogen is never center) 3. draw bonds and subtract those from total 4. assign remaining to terminals and subtract 5.if left over add to center and make multiple bonds if hasn't reached octet |
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what happens if there are multiple ways to make a lewis drop structure of a molecule ? |
the structure with the lowest formal charges are favored in nature |
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how do you find formal charge? |
valence electrons - associated electron = formal charge |
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what is the octet rule? |
atoms in the molecules should have 8 electrons associate with them |
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What are some exceptions to the octet rule? |
if there are an odd number of electrons then it could have fewer than 8 electrons. if the central atoms have d orbitals then it can have an expanded octet |
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what is electronegativity |
is is the amount an atom wants to attract atoms |
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what is polarity |
polarity in bonds is when one molecule wants attract the electrons more than the other causing there to be an negative side and a positive side (higher electronegativity) polarity in molecules is when the polarity of the bonds don't balance out. |
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how do you represent polarity |
1. having a sigma- charge over the one with more electronegativity and a sigma+ charge over the other 2. having a plus sign over the least electronegative and having it point to the negative side |
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equation for dipole moment |
u = Q x r |
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if the terminal atom are similar on a molecule how do you figure the polarity |
molecule with no lone pairs are non polar molecules with lone pairs are almost always polar ( check tho) |
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what is the molecular geometry, hybridization and angles for 2 electron domains |
linear, sp, 180
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what is the molecular geometry, hybridization and angles for 3 electron domains |
Trigonal Planar, sp2, 120
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what is the molecular geometry, hybridization and angles for 4 electron domains |
Tetrahedral, sp3, 109.5
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what is the molecular geometry, hybridization and angles for 5 electron domains |
Trigonal Bipyramid, dsp3, 180, 90, 120
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what is the molecular geometry, hybridization and angles for 6 electron domains |
Octahedral, d2sp3, 90, 180
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what are some of the deviations from expected angles in molecular geometry |
1. lone pairs take up more space than single bonds 2. multiple bonds repel more than single bonds |
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what are intermolecular forces? |
they are forces that interested between different molecules |
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what are the intermolecular forces in order from strongest to weakest? |
Electrostatic >> ion-dipole >> hydrogen bonding >> dipole dipole>> london dispersian |
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what are electrostatic intermolecular forces ? |
these are ionic bonds that are the strongest because the atoms have full bonds |
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what are ion- dipole intermolecular forces? |
these involves and ion and dipole molecule and are second strongest because it involves a full charge and a partial charge |
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what are hydrogen bonding intermolecular interactions |
these are very strong dipole -dipole interactions. they are strong because they involve hydrogen and an atom with a high electronegativity making the difference huge and a strong dipole dipole |
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what are dipole - dipole intermolecular interactions ? |
this involve partial charges between two molecules and thats what makes them weaker than the other but stronger than london dispersion |
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what are long dispersion intermolecular interactions ? |
all covalent molecules have this it consists of the theory that there is a possibility of all the electrons to be on one side of the molecule for a split second making it polar |
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how to figure out the polarity of a molecule |
the polarity is the difference of the electronegativity if the electro negativity is... less than .5 : it is non polar covalent between .5-2: it is polar covalent greater than 2: it is ionic |
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What is Valence bond Theory |
a covalent bond forms from the overlap of the half filled orbitals containing unpaired electrons with opposite charges. is the orbitals are different like s and p then they take the wave functions and combine them and this is called hybridization |
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what is Molecular Orbital Theory |
a covalent bond forms when two atomic orbitals for to create molecular orbitals, bonding and non bonding |
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what is bond order and how do you find it ? |
bond order tells if the molecule in molecular orbital theory is stable and you find it with bond order = (bonding - non bonding)/2 any number over 0 is stable |
