Exam 2 – Chemistry – Flashcards
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| binary ionic compound |
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| contain two elements; metal and nonmental |
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| aqueous solution |
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| when a compound dissolves in water |
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| ternary ionic compounds |
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| contains (3) elements; with at least one metal and one nonmetal |
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| binary molecular compound |
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| contain two elements that are both nonmetals |
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| binary acid |
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| an aqueous solution of a compound containing hydrogen and one nonmetal |
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| ternary oxyacid |
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| an aqueous solution of a compound containing hydrogen, a nonmetal and oxygen |
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| a positive ion |
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| cation |
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| a negative ion |
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| anion |
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| Iron's ions |
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| 2+, 3+; Iron (II); Iron (III) |
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| copper's ions |
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| + and 2+; Copper (I); Copper (II) |
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| What is the stock system? |
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| Naming transitional metal cations |
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| Latin system |
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| naming metal cations having two common ionic charges |
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| metals tend to form _____ ions |
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| positive |
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| nonmetals tend to form ______ ions. |
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| negative |
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| metal ions are named by... |
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| latin root and lower charge receives -ous and higher recieves -ic |
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| nonmetal ions are named by .... |
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| taking the stem and adding the suffix -ide. |
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| tin's ions |
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| 2+ and 4+; Tin(II) and Tin(IV); Sn |
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| lead's ions |
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| 2+ and 4+; Lead(II) and Lead(IV); Pb |
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| cobalt's ions |
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| 2+ and 3+; Coblat(II) and Cobalt(III); Co |
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| mercury's ions |
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| 2+ and Hg2^2+; |
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| isoelectronic |
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| becoming isoelectronic with another group in the periodic table because of a loss or gain of electrons. |
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| When a polyatomic anion consists of one or more elements and oxygen it is referred to as: |
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| oxyanion |
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| an example of an oxyanion |
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| NO3^- (nitrate ion) |
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| When a polyatomic anion has two forms, the one with more oxygen atoms ends with a _____ and the one with less ends with _______. |
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| -ate; _ite |
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| Nitrite ion |
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| NO2^- |
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| CN- |
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| Cyanide ion |
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| OH- |
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| hydroxide ion |
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| hydroxide ion |
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| OH- |
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| cyanide ion |
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| CN- |
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| NH4+ |
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| Ammonium ion (cation) |
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| Most oxyanions have the suffix: |
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| -ate |
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| formula unit |
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| the simplest representation particle in an ionic compound; |
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| what charge is a formula unit? |
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| Neutral |
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| Aluminum Ion |
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| AL 3+ |
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| Barium Ion |
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| Ba 2+ |
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| Cadmium ion |
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| Ca 2+ |
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| Cobalt (II) ion |
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| Co 2+ |
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| Cobalt (III) ion |
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| Co 3+ |
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| Copper (I) ion |
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| Cu + |
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| Chromium (III) ion |
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| Cr 3+ |
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| Hydrogen ion |
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| H+ |
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| Iron (II) ion |
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| Fe 2+ |
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| Iron (III) ion |
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| Fe 3+ |
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| Lead (II) ion |
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| Pb 2+ |
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| Lead (IV) ion |
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| Pb 4+ |
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| Lithium Ion |
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| Li + |
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| Magnesium ion |
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| Mg 2+ |
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| Manganese (II) ion |
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| Mn 2+ |
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| Mercury (I) ion |
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| Diatomic(Hg2) 2+ |
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| Mercury (II) ion |
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| Hg 2+ |
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| Nickle (II) ion |
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| Ni 2+ |
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| Potassium ion |
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| K+ |
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| Silver Ion |
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| Ag+ |
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| Sodium ion |
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| Na + |
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| Strontium ion |
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| Sr 2+ |
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| Tin (II) ion |
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| Sn 2+ |
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| Tin (IV) ion |
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| Sn 4+ |
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| Zinc ion |
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| Zn 2+ |
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| Bromide ion |
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| Br - |
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| Chloride ion |
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| Cl- |
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| Fluoride ion |
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| F- |
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| iodide ion |
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| I- |
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| nitride ion |
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| N 3- |
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| Oxide ion |
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| O 2- |
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| Phosphide ion |
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| P 3- |
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| Sulfide ion |
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| S 2- |
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| acetate ion |
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| C2H3O2- |
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| carbonate ion |
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| CO3 2- |
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| Chlorate ion |
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| ClO3- |
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| Chlorite ion |
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| ClO2- |
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| Chromate ion |
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| CrO4 2- |
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| cyanide ion |
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| CN- |
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| Dalton model of atom |
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| Proposed all atoms are composed of small paticles |
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| What two scientific principals did Dalton rely on to come to his conclusion about atoms? |
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| The law of conservation of mass and the law of definite composition |
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| Who established the law of conservation of mass? |
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| Lavoisier |
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| Who established the law of definite composition? |
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| Proust |
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| What did Dalton discover? |
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| The existence of atoms |
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| Dalton proposed that the charge of every atom was... |
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| neutral |
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| Thomposon's model of the atom was considered to be similar to what shape? Why? |
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| Plum pudding; because the electrons and protons were similar to the plums and the sphere would be the pudding. |
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| What experiment did Thompson use to help him determine his theory? |
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| Cathode ray tube |
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| Who calculated, named and determined the charge of an electron? |
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| Thompson |
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| Rutherford is known for his experiments using... |
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| radiation; alpha ray and beta ray |
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| Which type of radiation is not affected by a magnetic field? |
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| Gamma ray |
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| Rutherford is known for the.... |
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| nucleus. He defined that an atom has electrons around a nucleus which housed the protons |
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| Alpha rays are composed of |
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| helium atoms that have been stripped of their electrons |
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| Rutherford proposed the mass of the_____ was larger in comparison to the electrons. |
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| Nucleus |
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| In the gold foil experiment, what was discovered? |
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| that the atom has a larger nucleus and the alpha particles were reflected because of the dense positively charged nucleus of the gold |
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| The atomic number is the number of |
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| protons |
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| mass number |
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| neutrons + protons |
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| What is a shorthand way of determining # of neutrons? |
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| mass number - atomic number = neutrons |
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| The number of ______ determines what the element will be. |
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| Protons |
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| Where is the atomic number located when using atomic notation? |
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| The lower left hand corner of element symbol |
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| The higher the frequency the ______ the energy |
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| higher |
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| In the visible light scale, the frequency of wavelength go from _____ to ______ when looking from violet to red. |
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| high to low |
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| What is a photon? |
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| An individual energy of light |
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| "s" sublevel holds a max of ____ electrons |
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| 2 |
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| "p" sublevel holds a max of ____ electrons. |
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| 6 |
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| The "d" sublevel holds a max of ___ electrons. |
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| 10 |
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| The "f" sublevel holds a max of ___ electrons. |
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| 14 |
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| When drawing the electrons for the electron dot formulas, the ________ is in the middle and the _________ electrons are drawn. |
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| atomic symbol; valence. |
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| the horizontal portion of the periodic table are called: |
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| Periods |
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| how many p orbitals are there? |
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| 3; each hold two electrons per orbital |
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| what is the shape of the p orbitals? |
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| dumbbell |
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| What is a wavelength? |
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| The distance the light wave travels to complete one cycle. |
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| frequency |
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| number of wavelength refers to the number of wave cycles completed in each second. |
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| What did Niels Bohr discover about the atom? |
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| That electrons travel in a fixed-energy orbit/ energy level. |
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| When an electron is excited it moves from______. |
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| a higher energy level and back to a lower energy level |
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| When is a photon emitted? |
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| Each time an electron drops to a lower level |
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| A + B ---> AB |
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| Combination reaction |
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| AB ----> A + B |
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| Decomposition Reaction |
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| A + BZ ---> AZ + B |
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| single-replacement reaction |
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| AX + BZ ---> AZ + B |
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| double-replacement reaction |
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| HX + BOH ---> BX + HOH |
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| Neutralization reaction |
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| On the activity series, when a metal is above another in the series, the metal below is more or less likely to react with the one above? |
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| The metal below is less likely to react because it is lower on the series. The higher the metal on the series, the more reactive |
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| What are the seven diatomic molecules? |
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| Br2; Cl2; F2; H2; I2; N2; O2 (Brown Cloud Farts Happen I N Oklahoma) |
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| Niels Bohr's model of the atom: |
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| electrons circling around the nucleus in fixed-energy levels |
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| the vertical portion of the periodic table is called: |
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| groups or families |
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| Within a group or a period are elements similar in their chemical behavior? |
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| In a group because of the electrons (same amt. of valence) |
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| How many electrons are in the 3rd energy level? |
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| 18 because 3s; 3p; 3d. s holds 2; p holds 6; and d holds 10. |
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| How are the p orbitals situated in regards to the nucleus and eachother? |
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| They intersect the nucleus and are oriented at right angles to each other. |
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| What can be said about s orbitals, especially their relative size to one another? |
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| That 1s will be much smaller in size tan 3s. |
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| What shape are s orbitals? |
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| sphere |
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| What can be said about an electron orbital? Is it sure that we will find an electron there? |
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| When speaking of electron orbitals, there is a higher probability that we will find an electron there. |
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| ionization energy refers to: |
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| the amount of energy needed to remove an electron in the gaseous state |
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| Ionization energy increases as you go from _________ to _______ in the period. |
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| Left to right; bottom to top |
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| The atomic radius increases as we go ______ to ______ on the periodic table. |
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| bottom; top in a group right to left (row) |
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| Metallic character increases as you go _____ to ______ across a period and ______ to ________ across a group. |
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| right to left across a period top to bottom across a group |
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| The left side of the periodic table tend to be _________. |
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| Metals |
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| The right side of the periodic table tend to be _________. |
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| nonmetals |
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| Where are the noble gases located on the periodic table? |
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| Group 18, the last column |
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| Where are the representative elements located? |
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| To the left and right of the transitional metals. The groups with A |
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| Where are the transitional metals located? |
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| the middle of the periodic table. |
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| Where are the chemical behaviors of the elements most predictable? |
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| The representative elements |
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| Where is the lanthanide series? |
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| They are located with the inner transition elements that begins with lanthanide. |
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| Where is the actinide series? |
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| They are located in the inner-transition metals as a second part after the lanthanide series. |
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| Where are the halogens located? |
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| They are group 17 the second group from the left. |
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| Where are the alkali metals? |
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| The first group. The first column of the periodic table. |
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| Where are the alkali earth metals located? |
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| They are group 2 in the periodic table. The second column. |
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| When naming binary molecular compounds, what system is used? |
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| You must use the greek prefixes which refer to the number of atoms present in the compound. |
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| What is the Greek prefix for 4? |
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| tetra |
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| what is the Greek prefix for 5? |
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| Penta |
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| What is the Greek prefix for 10 |
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| deca |
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| what is the Greek prefix for 6? |
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| hexa |
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| What is the Greek prefix for 7? |
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| Hepta |
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| what is the Greek prefix for 9? |
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| Nona |
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| When naming binary ionic compounds, what must occur before the naming begins? |
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| There must be neutral atoms and the equation must be balanced. |
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| Sulfate ion |
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| SO4 2- |
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| Hypochlorite ion |
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| ClO- |
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| Phosphate ion |
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| PO4 3- |
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| Sulfate ion |
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| SO4 2- |
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| Sulfite ion |
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| SO3 2- |
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| How many moles would equal Avogadro's number? |
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| 1 |
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| What is the molar mass of a substance? |
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| atomic mass of a molecule given in grams. g/mol = MM |
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| What is the molar volume of a gas at STP? |
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| 22.4 L |
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| One mole of gas |
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| 22.4 L |
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| How do you calculate gas' density @ STP? |
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| the formula's mass/ 22.4L |
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| What are the steps of percent composition? |
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| First, find out the molar mass of the compound. Then take each individual weight take it over the overall weight multiplied by 100%. Always equals 100. |
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| How do you find the empirical formula when you work with percent composition? |
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| You wold take the smallest value and put all the values on the numerator with the smallest value in the denominator. |
