Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
ChemCards
Chemistry study cards
| Term | Definition |
|---|---|
| 1 amu | 1.66054×10^−24 g |
| 1 g | 1.66054×10^−24 g |
| Atomic weight | Atomic weight =∑over allisotopes ofthe element[(isotope mass) × (fractional isotope abundance)] |
| Naturally occurring carbon, for example, is composed of 98.93% ^12C and 1.07% ^13C. The masses of these isotopes are | 12 amu (exactly) and 13.00335 amu, respectively, making the atomic weight of carbon (0.9893)(12 amu)+(0.0107)(13.00335 amu)=12.01 amu |
| Two isotopes of boron are found in nature: 10B has a mass of 10.01 amu, and 11B has a mass of 11.01 amu. Use the atomic weight of boron found in the periodic table to determine which isotope is more abundant, 10B or 11B. | The atomic weight of boron, 10.811 amu, is closer to 11B which means 11B is the more abundant isotope. |
| Naturally occurring chlorine is 75.78% 35Cl (atomic mass 34.969 amu ) and 24.22% 37Cl (atomic mass 36.966 amu ). Calculate the atomic weight of chlorine. | Atomic weight = =(0.7578)(34.969 amu)+(0.2422)(36.966 amu) = 26.50 amu + 8.953 amu = 35.45 amu The atomic weight, average atomic mass, is between the masses of the two isotopes and is closer to the value of 35Cl, the more abundant isotope. |
| Write the empirical formulas for glucose, a substance also known as either blood sugar or dextrose—molecular formula C6H12O6. | Subscripts of empirical formula = smallest whole-number ratios. Smallest ratios = dividing each subscript by the largest common factor, = 6. Empirical formula for glucose = CH2O. . |
| Write the empirical formulas for nitrous oxide, a substance used as an anesthetic and commonly called laughing gas—molecular formula N2O. | Since subscripts in N2O = lowest integral numbers, empirical formula for N2O = molecular formula, N2O |
| Give the chemical symbol, including superscript indicating mass number, for the ion with 22 protons, 26 neutrons, and 19 electrons | # protons = atomic # of element. The element with atomic number 22 is titanium (Ti) . The mass # (protons + neutrons) of this isotope of Ti is 22+26=48. Because the ion has 3 more protons than electrons, it has a net charge of 3+ and is ^48Ti^3+. |
| Give the chemical symbol, including superscript indicating mass number, for the ion of sulfur that has 16 neutrons and 18 electrons. | Sulfur (S) has an atomic number of 16. Each atom or ion of S contains 16 protons. The ion has 16 neutrons, meaning the mass number = 16+16=32. Because the ion has 16 protons and 18 electrons, its net charge is 2− and the ion symbol is ^32S^2−. |
| What is the empirical formula of the compound formed between W^6+ and O^2–? | WO^3 |
| What information is conveyed by the endings -ide, -ate, and -ite in the name of an anion? | The endings convey the number of oxygen atoms bound to the nonmetallic element |
| What information is conveyed by the endings -ide, -ate, and -ite in the name of an anion? | The endings convey the number of oxygen atoms bound to the nonmetallic element |
Created by:
rpkw0000