Modern Chemistry – Holt Chapter 7 – Flashcards
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chemical formula
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subscript of each element reveals number of atoms contained in a single molecule of a certain compound
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monoatomic ions
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ions formed from a single atom; remember to change nonmetals to -ide ending
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oxyanions
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polyatomic ions that contain oxygen
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binary ionic compounds
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compounds of 2 elements between metal (positive, s-block and p-block) and nonmetal (negative); metal is always listed first; change nonmetal to -ide ending
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Stock system
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specifically used for d-block elements, use Roman numeral to describe charge of metal, use periodic charge to find charge of nonmetal
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Greek prefixes
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used to name molecules w/covalent bonds
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binary molecular compounds
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nonmetal to nonmetal; covalent bonds; Greek prefixes
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formula mass
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sum of all atomic masses of elements present in formula of compounds
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percentage composition
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percentage by mass of each element in a compound
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empirical formula
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symbols for elements combined in a compound; subscripts show smallest whole-number mole ratio of different atoms in a compound
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What is a mole?
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SI unit used to measure the amount of a substance. 12 g carbon
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how much mole is/molar mass
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atomic weight or 6.022...
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1 mole of h2o how many moles of hydrogen?
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2 moles
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diff between average atomic and molar mass and atomic mass units(protons and neutrons)
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atomic mass is the mass of 1 atom of a particular element and molar mass is the mass of 1 mole of an atom or molecule
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how many atoms in 1 mole of water?
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6.022X10^23 X 3
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polyatomic anion
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multiple atoms with an overall negative charge
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molar mass=
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g/mole
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average atomic mass of magnesium.
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50% 38 amu. 50% 20 amu. 50X38. 50X20Add them all together
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find the number of molecules in 2.5 mol. of sulfur dioxide
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2.5 mol SO2 X 6.022=
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3.01 X 10 ^23 molecules of sulfur dioxide, SO2. Determine the amount in moles
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3.01 X 10^23 molecules SO2 / 6.022=
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Find mass in grams of 2.44 X 10^24 atoms of carbon, whose molecular mass is 12.01 g/mol
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2.44 / 6.022 X 12.01gC=
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Find number of molecules present in 47.5 g of glycerol, C3H8O3. The molar mass of glycerol is 92.11 g/mol
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47.5g / 92.11 X 6.022=
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Find the mass of barium nitrate
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multiply molar mass by number of moles and add total
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percent to empirical formula
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% / molar mass. take smallest and / answers
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the empirical formula for a compound is P2O5. its experimental molar mass is 284 g/mol. determine the molecular compound
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molar mass of P X 2. molar mass of O X 5. = 141.94. 284 / 141.94 =
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calculate the percentage composition of copper (I) sulfide, a copper ore called chalcocite
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molar mass Cu X 2 + molar mass S X 1= 159.17. Cu/ 159.17= % Cu... etc.
