Term
| Rutherford's Gold Foil Experiment |
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Definition
| bombarded positively charged particles (alpha particles) at a piece of gold foil and recorded the angles at which they rebounded to find the composition of an atom |
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Term
| what is the ratio of electrons to protons in a neutrally charged atom? |
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Definition
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Definition
| number of protons in the nucleus |
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Definition
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Definition
| an atom of that element with a different mass number (different number of neutrons) |
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Term
| if Boron-11 is an isotope of Boron-10, how many neutrons does Boron-11 have? |
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Definition
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Term
| why will an ice cube made of deuterium not float in water? |
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Definition
| deutrium is an isotope of hydrogen with two neutrons instead of two, so it's heavier than normal ice. |
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Term
| what is the chemical difference between isotopes of the same element? |
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Definition
| no chemical difference - only the mass is different. |
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Term
| with what units do you measure atomic mass? |
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Definition
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Term
| why is the weight of an element not going to be exactly the same as its mass number? |
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Definition
| it's a weighted average according to how much of each isotope exists |
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Term
| what is the most abundant isotope of carbon? |
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Definition
| carbon-12 (closest number to its weight on the periodic table) |
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Term
| if Boron is 20% Boron-10 and 80% Boron-11, how do we figure out its average mass? |
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Definition
| .20(10.00) +.80(11.00) = average mass |
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Term
| what is the unit for counting atoms or molecules? |
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Definition
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Term
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Definition
| 6.022e23 --> the amount of particles in a mole (any substance) |
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Term
| if 1 carbon atom weighs 12amu, how much does a mole of carbon weigh? |
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Definition
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Term
| if a mole of hydrogen is 1 gram, how much does 1 atom of hydrogen weigh? |
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Definition
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Term
| 2 helium atoms are 8 amu, so how much is 1 mole of helium? |
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Definition
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Term
| rows in the periodic table |
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Definition
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Term
| columns in the periodic table |
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Definition
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Term
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Definition
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Term
| characteristics of metals (5) |
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Definition
- conduct heat and electricity
- malleable
- ductile
- luster
- solids at room temperature (except for mercury, which is a liquid) |
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Term
| where are nonmetals on the periodic table? |
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Definition
| to the right of the staircase |
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Term
| what is the one nonmetal that is liquid at room temperature? |
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Definition
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Term
| where are the metalloids? |
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Definition
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Term
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Definition
| Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium |
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Term
| how well do metalloids conduct? |
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Definition
| decent semiconductors (better when heated) and good conductors when doped (small amount of impurity added) |
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Term
| what state are metalloids? |
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Definition
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Term
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Definition
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Term
| Chemistry is the study of: (2) |
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Definition
- matter
- the reactions that transform one type of matter into another |
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Term
| chemists are involved in either: (a) |
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Definition
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Term
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Definition
| examining what something is |
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Term
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Definition
| creating/improving something new -- drugs, etc |
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Term
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Definition
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Definition
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Term
| pure substance vs. mixture |
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Definition
pure substance: can't be broken down by physical change
mixture: CAN be broken down by physical change |
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Term
| two kinds of pure substances |
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Definition
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Term
| homogeneous mixtures vs. heterogeneous mixtures |
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Definition
homogeneous mixtures: uniform throughout on a molecular level
heterogeneous mixtures: not uniform throughout |
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Term
| another word for a homogeneous mixture |
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Definition
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Term
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Definition
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Term
| heterogeneous mixture ex: |
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Definition
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Term
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Definition
| elements CANT be broken down by chemical change; compounds CAN |
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Term
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Definition
| transformation of one substance into another |
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Definition
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Definition
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Term
| the properties of compounds are ___________, and ______________ from the elements they are composed of. |
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Definition
| the properties of compounds are UNIQUE and DIFFERENT from the elements they are composed of. |
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Term
| ex: compound with different properties than its compositional elements |
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Definition
| hydrogen gas is explosive, water is not |
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Term
| key difference between elements and compounds |
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Definition
| compounds can be broken down by chemical means; elements CAN'T |
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Term
| does the order in which elements combine in a compound matter? |
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Definition
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Term
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Definition
| color, melting/boiling point |
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Term
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Definition
| how a substance reacts/relates to other substances |
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Term
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Definition
| how a substance reacts/relates to other substances |
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Term
| qualitative vs. quantitative properties |
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Definition
qualitative: can't measure (color, hard/soft, etc.)
quantitative: CAN measure (mass, density, etc) |
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Definition
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Definition
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Definition
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Definition
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Term
| SI unit: amount of a substance |
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Definition
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Term
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Definition
| two or more units together -- ex: meters/second^2 |
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Term
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Definition
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Term
| more density is _________ mass in _________ volume |
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Definition
| more density is MORE mass in LESS volume |
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Term
| intensive property vs extensive property |
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Definition
intensive property: doesn't matter how much you have, property howdoesn't change
extensive property: depending on how much of the substance you have, property changes |
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Term
| how are temperature scales defined? |
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Definition
| set two points; find temperature between them (ie. freezing point of water -- boiling point of water) |
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Term
| what is zero degrees on the Kelvin scale? |
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Definition
| absolute zero - where all particles stop moving (lose all their energy) |
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Term
| how do you convert Celsius to Kelvin? |
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Definition
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Term
| how many significant figures? 10.15 |
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Definition
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Term
| how many significant figures? .0015 |
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Definition
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Term
| how many significant figures? .00150 |
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Definition
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Term
| rewrite, margin of error, and significant figures: 3x10^2 |
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Definition
300
- 1 significant figure
- margin of error is 100 |
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Term
| margin of error, scientific notation, significant figures: 300.0 |
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Definition
- +/- .1
- 3.000x10^2
- 4 significant figures |
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Term
| how do you add and subtract numbers? |
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Definition
| answer has the same number of DECIMAL PLACES as component figure with fewest |
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Term
| how do you multiply and divide? |
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Definition
| answer has the same amount of SIGNIFICANT FIGURES as the component number with fewest |
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Term
| exact numbers (ex: number of seconds in a minute) are treated as if they have how many significant figures? |
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Definition
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Term
| how did radioactivity prove that atoms are made from smaller particles? |
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Definition
| observed atoms spontaneously breaking up into smaller pieces |
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Term
| Thompson's Cathode Ray Tube Experiment determined: |
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Definition
| the charge to mass ratio of an electron |
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Term
| Thompson's Cathode Ray Tube Experiment consisted of |
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Definition
| charged plates at opposite ends of a glass vacuum tube -- manipulating the resulting stream of electrons using magnetic fields, proving they had mass and charge |
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Term
| Millikan's Oil Drop Experiment determined: |
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Definition
| the exact mass and charge of an electron |
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Term
| Millikan's Oil Drop Experiment: |
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Definition
| fine droplets of negatively charged oil (using x-rays) into a chamber with a negatively charged floor and a positively charged ceiling until the droplets hovered |
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Term
| condensation: physical or chemical change? |
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Definition
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Term
| color change with bleach: physical or chemical change? |
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Definition
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Term
| Alkali metals react with water to produce: |
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Definition
| hydrogen and alkaline solutions |
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Term
| because of their reactivity, alkali metals are found in nature only in ___________ |
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Definition
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Term
| makes up 3/4 of the earth's atmosphere |
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Definition
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Term
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Definition
| making compounds from atmospheric nitrogen |
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Term
| what is a barrier to nitrogen fixation? |
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Definition
| need extreme conditions (like high temperatures) in a lab |
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Term
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Definition
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Term
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Definition
| sulfur, selenium, tellurium |
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Term
| halogens all exist as ________ molecules |
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Definition
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