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Chem exam 1 terms
Chem 109 exam 1
| Question | Answer |
|---|---|
| element | A substance that contains identical particles that consist of only one type of atom, can't be broken down |
| compound | a substance that contains identical particles; each particle consists of two or more different atoms, can be broken down |
| mixture | substance composed of two or more components in proportions that can vary |
| intensive properties | independent of sample size, used to identify substances Ex: color, density, boiling point |
| extensive properties | depends on sample size Ex: volume and mass |
| physical properties | property that a substance displays without changing its composition |
| mass | measure of quantity of matter |
| weight | force of gravity exerted on an object |
| atoms | most basic unit of matter |
| molecules | contains two or more atoms |
| pure substance | made of only one component |
| homogenous mixture | made of multiple substances but appears as one |
| heterogenous mixture | composition varies from one region of mixture to another |
| chemical properties | property that a substance displays only by changing its composition |
| physical change | no new substances formed, but substance may change state or proportions |
| chemical changes | formation of new substance, changes chemical makeup, new substance has different physical properties |
| quantitative measurement | measurements are expressed with a number |
| qualitative measurement | involves non-numeric data and are usually based on observations |
| unit equation | two equivalent quantities (2.54cm=1in) |
| conversion factor | (given x desired/given = desired) |
| Significant figure rules 1, 2, 3 | 1)Any nonzero digit is significant 2) Zeros between nonzero digits are significant 3) Zeros to the left of the first nonzero digit are not significant |
| Significant figure rules 4 and 5 | 4) Zeros to the right of the last nonzero digit are significant if a decimal is present. 5) Zeros to the right of the last nonzero digit in a number that does not contain a decimal point may or may not be significant. Best to use scientific notation |
| Significant figure rules addition/subtraction | In addition, and subtraction, the answer cannot have more digits to the right of the decimal point than any of the original numbers. |
| Significant figure rules multiplication/division | In multiplication and division, the number of significant figures in the final product or quotient is determined by the original number that has the smallest number of significant figures |
| accuracy | refers to how close the measured value is to the actual value |
| precision | refers to how close a series of measurements are to one another |
| How to calculate Kelvin from Celsius | K = C + 273.15 |
| How to calculate Fahrenheit from Celsius | F = (1.8 x C) + 32 |
| How to calculate volume | length x width x height (V = M/D) |
| How to calculate density | D = M/V |
| specific gravity | specific gravity = material density/water density |
| law | concise statement of a relationship between phenomena that is always the same under the same conditions; law is a summary |
| theory | unifying principle that explains a body of facts and/or those laws that are based on them; theory is an explanation |
| law of conservation of mass | mass is neither created nor destroyed in a chemical or physical change |
| law of constant proportions | compounds are composed of elements in certain fixed proprtions |
| law of multiple proportions | same elements, different compounds = mass ratios are whole numbers |
| law of combining values | ratio b/w the volumes of the reactant gases and products can be expressed in simple whole numbers |
| Avogadro's hypothesis | equal volumes of all gases under the same conditions of temperature and pressure contain the same number of molecules |
| isotopic symbols | x = atomic symbol of element a = mass # z = atomic number n = number of neutrons in nucleus |
| isotope | atoms of an elements have the same number of protons, but different number of neutrons |
| what is the charge of an atom | atoms have no net charge due to the equal number of electrons and protons |
| cation | positively charged ions |
| anion | negatively charged ions |
| how to calculate atomic mass | 1. list the isotopes of the element 2. convert each abundance to a decimal 3. multiply each isotopes mass by its decimal abundance 4. add all results together |
| isotopic abundance | percent abundance of each isotope of an element |
| properties of metals | metallic luster, malleable, ductile, hardness, conductive of heat and electricity, solid at room temperature |
| nonmetals | many are gas, some are solid, one is liquid, brittle, insulators |
| metalloids | b/w metals and nonmetals, metallic shine, brittle, semiconductors |
| heteronuclear molecules | molecule made of two or more different elements bonded together |
| homonuclear molecules | molecules made of only one kind of element |
| polyatomic molecules | contain more than two atoms |
| chemical formula | denotes the composition of the substance |
| structural formula | shows not only elemental composition but also general arrangments |
| molecular formula | shows the exact number of atoms of each element in a molecule |
| empirical formula | gives the simplest ratio of elements in a compound |
| ionic bonds | occurs b/w metals and nonmetals; involves the transfer of electrons from one atom to another |
| Do metals lose or gain electrons | lose |
| Do nonmetals lose or gain electrons | gain |
| polyatomic ions | charged groups of two or more atoms that stay bonded together and act as one ion |
| oxyanions | anions containing oxygen and another element |
| hydrates | compounds that have a specific number of water molecules within their solid structure |
| chemical bonds | occurs b/w two or more nonmetals involving the sharing of electrons between two atoms |
| organic compounds | carbon compounds |
| hydrocarbons | simplest organic compounds containing only C and H |
| acids | important class of molecular compounds that release hydrogen ions when dissovled in water |
| molecular mass | mass in atomic mass units of an individual molecule |
| How to calculate molecular mass | atomic mass x number of atoms of the element, then total the masses |
| formula mass | the mass in atomic mass unit of an ionic compound |
| How to calculate formula mass | multiply the atomic mass for each element in the empirical formula of ionic compound by the number of atoms of that element and then total the masses |
| law of constant proportions | compounds are composed of elements in certain fixed proportions |
| How to calculate percent yield | actual/theoretical x 100 = percent yield |
| What are the steps in balancing an equation | 1. write unbalanced equation 2. count atoms on each side 3. balance elements that appear in in only ONE compound on each side 4. use coefficients to balance atoms |
| How do we know if pairs are isotopes of the same element | if the bottom numbers match |
| percent composition of compounds | percent by mass of each element in a compound |
| How to calculate mole to particles | given x Avogadro's #/1 mole |
| How to calculate particles to moles | given x 1 mole/Avogadro's # |
| What is molar mass measured in | g/mol |
| What is atomic mass measured in | amu |
| How to calculate moles to mass | given moles x grams/1 mol |
| mass-mole-atom conversions | grams-molar mass-moles-Avogadro's #-particles |
| molar mass | mass of one mole of molecules of a compound; the mass of one mole of molecules in grams |
| molecular mass | mass of one molecule of a compound; this is the mass of one molecule in amu |
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