Chemistry Final Answers – Flashcards
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| Conversion of: Nanometers to meters |
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| x 10^-9 |
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| Conversion of: Micrometers to meters |
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| x 10^-6 |
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| Conversion of: Millimeters to meters |
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| x 10^-3 |
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| Conversion of: Centimeters to meters |
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| x 10^-2 |
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| Conversion of: Kilometers to meters |
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| x 10^3 |
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| Conversion of: Decameters to meters |
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| x 10 |
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| Conversion of: Megameters to meters |
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| x 10^6 |
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| Conversion of: Decimeters to meters |
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| x 10^-1 |
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| Conversion of: Hectometers to meters |
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| x 10^2 |
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| Conversion of: Gigameters to meters |
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| x 10^9 |
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| Conversion of: Celsius to Kelvin |
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| Kelvin = Celsius + 273 |
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| Conversion of: Fahrenheit to Kelvin |
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| (5/9 x (F - 32) + 273 ) |
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| Conversion of: Fahrenheit to Celsius |
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| (F - 32) x 5/9 = C |
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| Ammonium |
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| NH^4 |
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| Silicate |
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| SiO3^2- |
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| Dichromate |
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| Cr207^2- |
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| Oxalate |
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| C2O4^2- |
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| Permanganate |
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| MnO4^- |
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| Acetate |
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| C2H3O2^- |
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| Cyanide |
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| CN^- |
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| Hydroxide |
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| OH^- |
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| 1 mole of gas at STP = ________ L |
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| 1 mole of gas=22.4 L |
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| Avogadro's Number |
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| 6.02 x 10^23 |
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| Acronym for remembering polyatomic ions |
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| Nick the Camel ate Clam Crepes for Supper in Pheonix |
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| Hypo + polyatomic ion = ? |
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| 2 less Oxygen |
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| -ite + polyatomic ion = ? |
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| 1 less Oxygen |
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| Per + polyatomic ion = ? |
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| 1 more Oxygen |
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| Hydrogen + polyatomic ion = ? |
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| Add 1 to charge and add a H to front of symbol |
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| Naming binary ionic compounds |
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| 1. Cation first, then anion 2. Add -ide to anion 3. Balance charges |
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| Naming binary molecular compounds |
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| 1. Cation first, then anion 2. Use prefixes to indicate # of atoms of element 3. If 1st element has only 1 atom, then omit prefix 4. Add -ide to the anion |
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| Naming acids ending in -ide |
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| 1. Cation first, then anion 2. Begins with hydro- 3. Stem of anion ends in -ic 4. Followed by word "acid" |
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| Naming acids ending in -ite |
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| 1. Cation first, then anion 2. Anion ends in -ous 3. Followed by word "acid" |
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| Naming acids ending in -ate |
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| 1. Cation first, then anion 2. Anion ends in -ic 3. Followed by word "acid" |
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| Naming bases |
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| 1. Cation first, then anion 2. Balance charges |
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| Common diatomic compounds |
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| Br I N Cl H O F |
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| Ionization energy |
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| Energy needed to take an electron |
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| Electronegativity |
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| Tendency of an atom to attract electrons |
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| Calculating energy of light |
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| c=v? |
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| Discovered the electron |
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| JJ Thomson |
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| Dalton's atomic theory |
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| 1. Elements are made of atoms 2. Atoms of the same element are identical 3. Atoms of different elements can make compounds in definite ratios 4. Atoms separate, join, or rearrange to make a chemical change |
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| Miliken |
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| e (charge)/mass |
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| Discovered the neutron |
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| Chadwick |
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| Discovered the proton |
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| Rutherford |
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| Conducted the Gold-foil experiment |
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| Rutherford |
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| Democritus said that "____" |
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| Atoms are the smallest, indivisible thingie |
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| Periods are ____ |
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| rows |
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| Groups are _____ |
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| columns |
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| Atoms get their identity based on the number of _____. |
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| protons |
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| Atoms get their properties based on the number of ______. |
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| valance electrons |
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| Put the following in order based on largeness to smallness: Suborbit, Atom, Orbit/Energy level, Electrons, Orbitals |
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| Atom, Orbit/Energy level, Suborbit, Orbitals, Electrons |
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| Number of electrons in S |
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| 2 |
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| Number of electrons in P |
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| 6 |
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| Number of electrons in D |
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| 10 |
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| Number of electrons in F |
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| 14 |
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| Equation to find the number of maximum electrons in energy level (n=__) |
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| 2n^2 |
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| Aufbau Principle |
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| Electrons fill lower energy orbitals before filling higher energy orbitals |
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| Pauli's Exclusion Principle |
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| Orbitals can only have 2 electrons |
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| Hund's Rule |
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| Before you pair electrons, you have to put one electron in each orbital |
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| Exceptions to normal electron configurations |
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| Chromium and Copper |
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| c=___ |
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| speed of light (3.0 x 10^8 m/s) unit= meters/second |
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| v (nu)= ___ |
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| Frequency (unit= hertz) |
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| ? (lambda)=____ |
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| Wave length (unit= meters) |
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| Equation for Energy of a Photon |
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| Eph=vh |
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| h (Plank's constant)= _____ |
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| 6.626 x 10^-34 |
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| How do you find the atomic mass of isotopes? |
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| 1. Multiply each percent (of abundance) by the average mass and add all of the different isotopes together. 2. Divide by 100 |
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| Electronegativity __1__ from bottom to top, and ___2___ from left to right |
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| 1. increases 2. increases |
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| Ionization energy __1__ from bottom to top, and ___2___ from left to right |
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| 1. increases 2. increases |
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| Atomic size __1__ from bottom to top, and ___2___ from left to right |
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| 1. decreases 2. decreases |
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| Nonmetal + nonmetal = ? |
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| covalent bond |
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| Nonmetal + metal = ? |
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| ionic bond |
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| Metal + metal = ? |
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| metallic bond |
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| If electronegativity is between 0 and 0.4 the bond is _____ |
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| Nonpolar covalent |
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| If electronegativity is between 1.4 and 1 the bond is _____ |
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| Moderately polar covalent |
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| If electronegativity is between 1 and 2 the bond is ______ |
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| Very polar covalent |
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| If electronegativity is greater than or equal to 2 the bond is _____ |
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| Ionic |
