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 |
