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Stack #65101
| Chemistry | Unit 1,2 |
|---|---|
| Deci | (d) 10E-1 |
| Centi | (c) 10E-2 |
| Milli | (m) 10E-3 |
| Micro | (u) 10E-6 |
| Nano | (n) 10E-9 |
| K =? | K= C + 273.15 |
| C= ? | (5/9) (F-32) |
| F=? | (9/5)(C)+32 |
| Density=? | D=m/v |
| Volume=? | V=M/D |
| Mass=? | M=DV |
| Density of H20? | 1.00 |
| Sig Fig Rule #1 | zeros between nozero didgets are always signifiant |
| Sig Fig Rule #2 | zeros at the beggining of a number are never significant |
| Sig Fig Rule #3 | zeros at the end of a number are significant if the number contains a decimal |
| x and / for sig figs | result contains same number of sigfigs as the fewest measurement. (numbers are counted) |
| + and - for sig figs | result has same number of decimal places as the measurement with the fewest decimal places. (decimals have been counted) |
| carbon | C |
| Flourine | F |
| Hydrogen | H |
| Iodine | I |
| Nitrogen | N |
| Oxygen | O |
| Phosphorous | P |
| Sulfur | S |
| Aluminum | Al |
| Bromine | Br |
| Calcium | Ca |
| Chorine | Cl |
| Helium | He |
| Lithium | Li |
| Magnesium | Mg |
| Silicon | Si |
| Copper | Cu |
| Iron | Fe |
| Lead | Pb |
| Mercury | Hg |
| Potassium | K |
| Silver | Au |
| Sodium | Na |
| Tin | Sn |
| JJ Thompson | caluclated the charge-to-mass ratio of the electron |
| robert millikan | calculated the mass of an electron, by first developing the charge |
| electron charge | -1.6E-19 C |
| electron mass | 9.10E-28 |
| 2 things Rutherford discovered? | 1. small, dense, positive NUCLEUS. 2.) most of the atom is empty space |
| Protons | discoverd 1919 by Rutherford, are positively charged subatomic particles |
| Nuetrons | discoverd 1932 by Chadwick, neutral subatomic particles |
| Ions | electrically charged atoms (or groups of atoms) = polyatomic ions |
| Cations | positive ions. when a neutral atom loses electrons...becomes more positive |
| Anions | negative ions, when a neutral atom gains electrons..becomes more negative |
| Metals | tend to lose electons (be positive) just add (ion) |
| Nonmetals | are negative. named by using the root of the element plude "ide ion" |
| charge of a proton | 1.602E-19C |
| isotopes | atoms with identical atomic numbers (#of protons) but different mass numbers (different #'s of neutrons) |
| Properties of Metals | high thermal and electrical conductivity, malleability, ductility, has metalic luster |
| Properties of Nonmetals | brittle, may be powdery solids, or gases. |
| 7 Natural diatomic molecules | BrINClHOF (Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, and Fluorine |
| Group 1A | Alkali Metals (Li, Na, K, Rb, Cs, Fr) |
| Group 2A | Alkaline earth metals (Be, Mg, Ca, Sr, Ba, Ra) |
| Group 6A | Chalcogens (O, S, Se, Te, Po) |
| Group 7A | Halogens (F, Cl, Br, I, At) |
| Group 8A | Nobel Gases (He, Ne, Ar, Ke, Xe, Rn) |
| covalent bonds | bonds that shares electrons |
| Ionic bonds | bonds that occur between oppositely charged ions |
| Ionic compounds | usualy composed of metals and nonmetals |
| 3 steps for writing binary Ionic compounds | 1. determine charge of ions. 2) write cation first, followed by anion 3.) use subcripts to balance charges on the ions. |
| Naming binary Compounds from Formulas | 1.) name the cation (metal) 2.) follow with name of anion, using the root of the anion plus the suffix "ide" 3.) if the cation of an element has several ions of different charges use a Roman Numeral |
| the polyatomic ion we have to memorize | NH4 + |
| 1+ Ions | Ammonium, Cesium, Copper, Hydrogen, Lithium, Potassium, Silver, Sodium |
| NH4 | ammonium + |
| Cs | + |
| Cu | + |
| H | + |
| Li | + |
| K | + potassium |
| Ag | + silver |
| Na | + Sodium |
| Ba | 2+ Barium |
| Cd | 2+ Cadmium |
| Ca | 2+ calcuim |
| Cr, Co, Cu, Fe, Pb, Hg, Mn, Ni, Sn | all can be (II) |
| Zn | 2+ zinc |
| Al | 3+ aluminum |
| Cr III | 3+ chromium |
| Fe III | 3+ iron |
| C2H302 | Acetate - |
| Br | - bromide |
| ClO3 | chlorate - |
| Cl | - chloride |
| CN | -cyanide |
| H2PO4 | - hihydrogen phosphate |
| F | - Flouride |
| H | - Hydride |
| HCO3 | - hydrogen carbonate (bicarbonate) |
| HS03 | - hydrogen sulfate (bisulfate) |
| OH | - hydroxide |
| I | - iodide |
| NO3 | - nitrate |
| NO2 | - nitrite |
| ClO4 | - perchlorate |
| MnO4 | - permangnate |
| SCN | - thiocyanate |
| C03 | 2- carbonate |
| CrO4 | 2- chromate |
| HPO4 | 2-hydrogen phosphate |
| O | 2- oxide |
| O2 | peroxide 2- |
| SO4 | 2- sulfate |
| S | 2- sulfide |
| SO3 | 2-sulfite |
| AsO4 | 3- arsenate |
| PO4 | 3- phosphate |
| Oxyanions: | polyatomic ions containing oxygen have names ending in "ate"or "ite" |
| suffix for most common oxygenation of an element | -ate |
| suffix for oxyanion that has same charge but fewer oxgen atoms. | -ite |
| prefix indicating one more oxygen than (ate) | "per" |
| prefix indicating one oxygen fewer than "ite" | "hypo" |
| binary covalent compounds | pure substances that consist of two nonmetallic elements. |
| writing formulas for covalent compounds | 1.) write names of elements in order 2.) prefix indicates # of each kind of atom. |
| mon(o) | 1 |
| di | 2 |
| tri | 3 |
| tetr(a) | 4 |
| pent(a) | 5 |
| hex(a) | 6 |
| hept(a) | 7 |
| oct(a) | 8 |
| non(a) | 9 |
| dec(a) | 10 |
| Naming inorganic compounds | 1.) dont use mono with first word. 2.) use stem "ide" as suffix. 3.)final vowel in a prefix is dropped before a voewel in the stem name. |
| Acid anion | replacese "ide" with "ic" and add prefix "hydro" |
| Acid | (blank) |
| Acid = | hydrogen+halogen ion = acid |
| If acid ends in "ate" | change end to "ic" (no hydro) |
| if acid endsin "ite" | change end to "ous" |
Created by:
kell5765