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Chemistry Exam I
| Question | Answer |
|---|---|
| Pure or applied: development of the computer chip | applied |
| Pure or applied: Study of radiation | Pure |
| Pure or applied: Developing a fuel additive that improves milage | Applied |
| Pure or applied: Investigating the properties of silicon | Pure |
| an idea or explanation that you then test through study and experimentation | hypothesis |
| a well-supported, systematic explanation for observed facts or phenomena, built from tested ideas and evidence, not just a guess, though informally it can mean a hunch or idea | theory |
| a statement that describes an observable occurrence in nature that appears to always be true | scientific law |
| a standard or comparison point in an experiment that helps determine if the variable being tested had an effect | control |
| value that remains unchanged | constant |
| he factor that a researcher intentionally changes or manipulates in an experiment to observe its effect on something else | independent variable |
| the outcome or effect being measured in an experiment, which changes in response to the independent variable (the cause or what's manipulated) | dependent variable |
| the systematic study of the structure and behavior of the physical and natural world through observation, experimentation, and the testing of theories against the evidence obtained. | science |
| studies matter and its properties, composition, and transformations | chemistry |
| the process scientists follow to solve problems | scientific method |
| a group or a variable that is kept constant to serve as a standard for comparison | controlled experiment |
| the process of assigning a numerical value to a physical quantity by comparing it to a standardized unit | measurement |
| part of a decimal system of measurement based on the meter, kilogram, and second for length, mass, and time, | metric units |
| a way to express huge or tiny numbers concisely as a product of a number between 1 and 10 (the coefficient) and a power of 10 (the base) | scientific notation |
| the digits in a number that are known with certainty, plus the first digit that is estimated or uncertain | significant figures |
| Solid/liquid/gas: low KE, classified as a crystalline | solid |
| Solid/liquid/gas: compressible | gas |
| Solid/liquid/gas: high KE particles can spread out | gas |
| Solid/liquid/gas: fairly low KE, particles can move around each other but still touch | liquid |
| Physical or chemical: a balloon inflated in a cooled store expands in a hot car | physical |
| a liquid evaporates to a gas | physical |
| iron reacts with oxygen | chemical |
| a transition from a gas to liquid | condensation |
| a transition from liquid to gas at the boiling point | evaporation |
| a transition from liquid to solid | freezing |
| a transition from solid to gas | sublimation |
| a transition from liquid to gas below the boiling point and only at the surface | type of evaporation - vaporization |
| a transition from solid to liquid | melting |
| Describe energy and particles during a phase change | During melting or boiling, energy changes the particles’ bonds, not their temperature, so the substance stays the same temperature until the change is done. |
| Describe energy and particle motion when temperature increase. | When temperature goes up, particles move faster. They have more energy, so they jiggle, slide, or bump into each other harder. The hotter it gets, the faster the particles move. |
| dirt | homogeneous mixture |
| liquid nitrogen | element |
| gold bar | element |
| apple juice | solution |
| what's dissolved | solute |
| does the dissolving | solvent |
| Chemical/physical property: conducts electricity | physical |
| Chemical/physical property: decomposing road kill | chemical |
| Chemical/physical property: explosive | chemical |
| Chemical/physical property: sublimation of dry ice | physical |
| Chemical/physical property: corrosive | chemical |
| Chemical/physical property: grating cheese | physical |
| Chemical/physical property: dissolves in water | physical |
| Chemical/physical property: acid rain damage to marble | chemical |
| compare and contrast mixtures and compounds | Mixtures are two or more substances together but not joined, and can be separated physically. Compounds are elements chemically joined, with new properties, and need chemical reactions to separate. |
| What happens to particles at Absolute Zero? | At absolute zero, particles stop moving completely. They have no energy at all and are as still as possible. |
| all matter is made of tiny particles (atoms/molecules) in constant, random motion, with their energy related to temperature | kinetic molecular theory |
| the energy an object possesses due to its motion | kinetic energy |
| the energy needed to change a substance from a solid to a liquid at its melting point, without changing its temperature | heat of fusion |
| the heat required to convert one kilogram of the liquid into vapour at its boiling point without any change of temperature. | heat of vaporization |
| the heat required to convert one kilogram of the liquid into vapour at its boiling point without any change of temperature. | absolute zero |
| the absolute temperature scale where 0 K (absolute zero) is the point where particles have minimal thermal energy, and each Kelvin unit equals a Celsius degree change | Kelvin scale |
| Physical properties describe a substance's appearance or behavior without changing its identity (like color, density, melting point), while chemical properties describe how it reacts to form a new substance | Physical and chemical properties |
| A physical change alters appearance (shape, state) but not the substance's identity (like ice melting to water, still H₂O), while a chemical change creates a new substance with different properties | physical and chemical changes |
| a chemical reaction that sends out heat or light, making its surroundings feel warm or hot | exothermic |
| one that absorbs energy, usually heat, from its surroundings, making the surroundings feel cooler | endothermic |
| Proposed the existence of a dense, +charged nucleus after the gold foil experiment | Ernest Rutherford |
| Discovered positive charges in atoms | Ernest Rutherford |
| Proposed the existence of (-) charged electrons | JJ Thomson |
| Proved the existence of neutrons in 1932 | James Chadwick |
| Developed the model of the atom with electron orbits | Niels Bohr |
| Developed the idea of an atom thousands of years ago | Democritus |
| Mendeleev arranged elements by_______________ | by increasing atomic mass and noticed that elements with similar properties appeared in patterns, which helped him create the first periodic table |
| Mosely arranged them by___________________ | by increasing atomic number, which fixed the problems in Mendeleev’s table and is how the modern periodic table is organized. |
| The tendency to attract and hold electrons is called | electronegativity |
| which has a larger radius Li or N? | N |
| which has a larger radius Ne or Xe | Ne |
| Which has a higher ionization energy: Li or Cs? | Li |
| Which has a higher electronegativity: Na or K | Na |
| List the subatomic particles & isotope symbol for bromine-80 | Protons (p⁺): 35 (same as the atomic number of bromine) Electrons (e⁻): 35 (neutral atom) Neutrons (n⁰): 80 − 35 = 45 Isotope symbol: 35 80 Br 35 80 Br |
| Calculate the average atomic mass of lithium if 1 of 13 atoms is lithium-6 & the other 12 atoms are lithium-7 | Step 1: Find the fractional abundance Step 2: Multiply each isotope by its fraction Step 3: Add them together 0.4615+6.4615≈6.923 |
| Will a metal form a cation or anion? | cation |
| Will a nonmetal form a cation or anion? | anion |
| Which element as the highest electronegativity? | Fluorine |
| What would the charge on an ion of Ca be based on valence electrons? | 2 valence electrons |
| Why do Noble Gasses not react? | their outer shells are full, so they’re already stable. |
| a version of a chemical element where atoms have the same number of protons but a different number of neutrons, resulting in different atomic masses but nearly identical chemical properties | isotope |
| the weighted average mass of all naturally occurring isotopes of an element | average atomic mass |
| the electrons in the outermost shell of an atom, and they are the ones involved in forming chemical bonds | valence electrons |
| the horizontal rows on the periodic table, showing elements with the same number of electron shells | period |
| a vertical column on the periodic table where elements share similar chemical traits because they have the same number of outer-shell (valence) electrons | group |
| shiny, malleable, ductile, and good conductors | metals |
| dull, brittle, poor conductors, often gases | nonmetals |
| have intermediate, hybrid properties, acting as semiconductors | metalloids |
| Groups 1, 2, and 13-18 of the periodic table | representative elements |
| elements in the middle of the periodic table (Groups 3-12) that are hard, shiny, good conductors, and often form colorful compounds | transition metals |
| two rows (lanthanides and actinides) usually at the bottom of the periodic table | inner trans metals |
| refers to the total count of protons and neutrons in an atom's nucleus | mass number |
| The rule that states most atoms form bonds to get 8 valence electrons | Octet Rule |
| Ionic or covalent: SO3 | covalent |
| Ionic or covalent: FeCl3 | Ionic |
| Ionic or covalent: NaNO3 | Ionic |
| How many atoms are in Ca(NO3)3 | Total atoms: 1 + 3 + 9 = 13 atoms |
| Ionic or Covalent form individual molecules | covalent |
| Ionic or Covalent: Involve the transfer of electrons | ionic |
| Ionic or Covalent: Form a crystal lattice structure of charged particles | ionic |
| Ionic or Covalent: Involve the sharing of electrons | covalent |
| Ionic or Covalent: Have a low melting point | covalent |
| Ionic or Covalent: Conduct electricity in a solution | Ionic |
| Polar or Nonpolar: usually formed between identical atoms | Nonpolar |
| Polar or Nonpolar involve the unequal sharing of electrons | Polar |
| Polar or Nonpolar: create partial + and - charges within the molecule | Polar |
| Polar or Nonpolar: Involve the equal sharing of electrons | Nonpolar |
| PCl₃, SO₂, N₂O₅ | Phosphorus Trichloride, Sulfur Dioxide, Dinitride Pentoxide |
| LiBr, MgSO₄, NaNO₂ | LIthium Bromide, Magnesium Sulfate, Sodium Nitrate |
| Write the molecular formulas for carbon tetrachloride, sulfur hexafluoride, dinitrogen monoxide | CCl₄. SF₆, N₂O |
| Write ionic formulas for: calcium chloride, aluminum oxide, copper (II) nitrate | CaCl₂, Al₂O₃, Cu(NO₃)₂ |
| Calculate the mass of Zn, | Zn is an element, so its molar mass = 65.38 g/mol |
| Calculate the mass of MgO | Mg = 24.31 g/mol O = 16.00 g/mol MgO = 24.31 + 16.00 = 40.31 g/mol |
| Calculate the mass of Ag₂CO₃ | Ag = 107.87 × 2 = 215.74 g/mol C = 12.01 g/mol O = 16.00 × 3 = 48.00 g/mol Ag₂CO₃ = 215.74 + 12.01 + 48.00 = 275.75 g/mol |
| a chemical principle stating that atoms tend to gain, lose, or share electrons to achieve a stable configuration with eight valence electrons | octet rule |
| molecules with an uneven distribution of electron density, creating distinct positive and negative ends (poles) due to differences in electronegativity between bonded atoms and the molecule's geometry | polar |
| a molecule has an even distribution of electrical charge, like a balanced seesaw, with no distinct positive or negative ends (poles) | nonpolar |
| seven elements that naturally exist as pairs of atoms (like H₂, N₂, O₂) for stability, not single atoms | diatomic elements |
| a chemical reaction where a substance loses electrons, often by combining with oxygen | oxidation number |
| a group of two or more atoms covalently bonded together that carries a net electric charge | polyatomic ion |
| involving ions (charged atoms or groups) held by strong electrostatic attraction, usually from a metal losing electrons to a non-metal, forming a stable, often crystalline compound like salt (NaCl) | ionic |
| when two atoms, usually nonmetals, share electrons to achieve a full, stable outer electron shell | covalent |
| an atom or molecule that gains one or more electrons, giving it a net negative charge, making it attracted to positive terminals (anodes) in an electric current | anion |
| an atom or molecule that has lost one or more electrons | cation |
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