Exam 1 – Chemistry Test Answers – Flashcards
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Hodson's Favorite element |
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Boron |
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What is a law? |
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A consistent observation |
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What is a theory? |
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Established hypothesis |
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Physical Properties are? |
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characteristic displayed by a sample of matter without undergoing any change in its composition e.g. color |
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Chemical Properties are? |
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characteristics displayed as a result of change in composition e.g. flammability |
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Physical Change |
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Not permeant, changes in appearance not composition |
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Chemical change |
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Change in composition |
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These are used to create a product |
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Reactants |
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Reactants create |
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A product |
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Matter is composed of? |
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Atoms |
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What is a substance? |
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A substance is a particular kind of matter with a fixed atomic composition that does not vary from sample to sample |
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What is an element? |
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a substance that cannot be broken down into any simpler substance by chemical means |
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What is a compound? |
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a substance made up of atoms of two or more elements, chemically combined, with the different kinds of atoms combined in fixed proportions |
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What is a heterogeneous mixture |
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A mixture that varies in composition |
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What is a homogenous mixture |
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a mixture containing a single substance, solution. |
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Solids are classified as |
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Crystalline (regular repeating pattern) and amorphous (no arrangement) |
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Important SI prefixes |
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Good Men Know Many More Numbers G 10^9 M10^6 k10^3 m10^-3 M10^-6 n10^-9 |
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Mass is |
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the amount of matter |
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weight is |
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the gravitational pull |
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What is temperature |
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the speed of motion of particles at a microscopic level |
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How do you measure Kelvin |
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Kelvin (K) = Celsius (?C) + 273.15 |
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How do you determine Fahrenheit? |
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Fahrenheit (?F) = [1.8 X Celsius (?C)] + 32 |
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1 ml = ____ cm? |
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1 cm^3 |
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1 cm^3 =? |
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I mL |
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Precision is? |
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How close measurements are to each other |
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Accuracy is? |
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How close the measurement is to the actual value |
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Density = |
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Mass/volume |
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What are the basic SI units? |
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kg, m, s, K, mol, A, Cd |
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The law of conservation of mass |
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Mass cannot be created nor destroyed |
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Law of Definite composition |
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Regardless of source, a particular compound is composed of the same elements in the same parts (fractions) by mass |
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Law of multiple Proportions |
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Different proportions of the same elements can create different substances |
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Who discovered atoms were divisible |
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JJ thompson, cathode ray |
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What was the rutherford experiment |
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Gold, atoms moving around, established the nucleus. |
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Mass number |
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Protons and neutrons |
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Atomic Number |
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Protons |
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Element symbol |
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for example Cl for cholorine |
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In order for an atom to be neutral |
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Protons and electrons must be equal |
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What is an Ion? |
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An ION is an ATOM or group of ATOMS which carries a net positive or negative charge |
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Cations |
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Positive Ion |
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Anion |
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Negative Ion |
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Isotope |
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Atoms of the same element (same Z) with different numbers of neutrons (different A) are ISOTOPES |
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Average Atomic Mass |
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Average Atomic Mass = ? (Fractional abundance ? atomic mass) for each isotope The Atomic Mass of an element is the weighted average relative mass of the isotopes of that element compared to the atomic mass of carbon-12, and is listed on the PERIODIC TABLE |
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Metals are |
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malleable, ductile, lustrous, high melting and boiling point, |
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Groups of metals |
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Alkaline metals, Alkaline earth metals, Transition metals and post transition metals |
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Nonmetal groups |
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other non metals, halogens and noble gases |
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The bottom group of the periodic table are the |
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Lanthanides and Actinides |
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A mole is |
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6.022 x 1023 |
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Molar Mass is |
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The atomic mass (u) of any element stated in grams (g) contains 1 mole (mol) of atoms of that element and is known as its MOLAR MASS (g/mol) |
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A diatomic molecule is |
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a molecule in an uncombined form. |
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What is empirical formula |
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the smallest whole number ratio of each type of atom in a compound |
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A structural formula shows....? |
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The covalent bonds between atoms in a molecule single bond, double bond, triple bond |
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What is an ionic compound? |
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Forms due to attractions, usually between a metal and a nonmetal |
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Molecular covalent bonds form between? |
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Non metals and Non metals |
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How do you find molar mass of a compound? |
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By adding the molar masses of each of the elements in the compound |
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Mass percentage composition? |
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tells us relative masses of elements combined in a compound |
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Molecular formula shows |
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the actual ratio, not a simplification |
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Can compounds have identical empirical formulas? |
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Yes |
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Calculating formula steps |
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mass percent of each compound grams of each elements moles of each element empirical formula |
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Calculating molecular and empirical formula |
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empirical formula * Integral factor = molecular formula |
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Organic compounds are formed from |
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C H N O P S |
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Ionic bond is between |
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metal and non metal Metal + nonmetal-ide |
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NH4+ |
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Ammonium |
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H3O+ |
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Hydronium |
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C2H3O2- |
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Acetate |
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CO3 2- |
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Carbonate |
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HCO3- |
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Hydrogen Carbonate |
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ClO- |
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Hypochorite |
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ClO2- |
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Chlorite |
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ClO3- |
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Chlorate |
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ClO4- |
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Perchlorate |
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CN- |
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Cyanide |
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OH- |
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Hydroxide |
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NO3- |
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Nitrate |
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NO2- |
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Nitrite |
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PO4 3- |
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Phosphate |
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PO3 3- |
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Phosphite |
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SO4 2- |
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Sulfate |
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SO3 2- |
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Sulfite |