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CHEM 130-90 LCCC
Chemistry Midterm Study
| Question | Answer |
|---|---|
| A 2.0 L bottle of soda has how many gallons of soda? | 0.53 gal (2 Sig fig) |
| An isotope of potassium (k19) has 19 protons 19 electrons and 21 neutrons. Its mass number and atomic number are, respectively.... | Atomic mass 40, Atomic number 19 |
| Does NOT apply to ionic bonding or ionic compounds. | Metals form the (-) ions while nonmetals form the (+) ions. |
| A football player weighs in at 275 lbs. How many grams? | 125000g 275lbs*1kg/2.2lbs*1000g/kg= |
| 1 gal | 3.78 L |
| What is the charge on an ion formed by an element in group 16? | -2 |
| Cs | Cesium |
| Sc | Scandium |
| S | Sulfur |
| Hg | Mercury |
| As | Arsenic Semi-metal (metalloid) |
| If the meniscus is between 22 and 23mL what is the measurement? | 22.6mL (watch sig sigs) |
| A graduated cylinder has marking at increments______smallest and _______largest. | 1mL 10mL |
| Form of chemical change | digestion |
| A 110lb woman is suppose to receive 3mg of medicine per kg of body mass, at 30mg per pill how many pills should she take? | 5 pills 110lb*1kg/2.2lb=50kg 50kg*3mg/1kg=150mg 150mg*1pill/30mg =5pills |
| Potassium | k 19 |
| Sulfur | S |
| Manganese | Mn |
| Mg | Magnesium |
| What compound is formed between iron(III) ion and the ion formed by Cl | FeCl3 |
| 38.5 inches | 0.978 meters |
| Chromium (II) phosphate? | Cr3(PO4)2 |
| Isotopes of a given element | different mass numbers, but same number of protons |
| How many electrons are in the outer shell of nitrogen? | 5 |
| In order to measure temp to 1/10th a degree (i.e. 17.5 degree C) the thermometer must have divisions at________ | 1 degree Celsius |
| CO3-2 (Polyatomic ion) | Carbonate |
| NO3-1 (Polyatomic ion) | Nitrate |
| SO4-2 (Polyatomic ion) | Sulfate |
| Normal body temp | 98.6 degree F |
| Does a child have a fever if temp is 306K? | No Less than 37 degree C = 91degree F 306K-273=33degreeC |
| Toxic dose is > 1.0 kg of body mass. The medication is supplied 150mL liquid. A 12kg child ingests 125mL is it toxic? | Yes it is toxic 125mL*150mg/mL = 18.75g = toxic >12g |
| If a kicker can kick 45meters he should be able to kick 45yards? T/F | True 1 meter = 1.09361 yard |
| Sodium Sulfide | Na2S |
| Nickel (III) hydroxide | Ni(OH)3 |
| Copper (II) Oxide | CuO |
| Calcium acetate | Ca(C2H3O2)2 |
| Be | 4 Beryllium 9 |
| Be has _____electrons Ne has _____ electrons Cl has _____ electrons | 2 8 7 |
| Round to 3 sig fig: 48.652, 10477, 8.00305 | 48.7, 10500, 8.00 |
| How many atoms in Ca(HCO3)2? | 11 atoms |
| How many atoms in Mn(OH)4 | 9 atoms |
| COCl2 | 2 single bonds, 1 double bond, planar triangular |
| Which reactant element is oxidized in the following reaction? Mg(s) + 2CuCl2(aq) ---MgCl2(aq) + 2Cu(s) | Mg |
| NaNO3 | Sodium nitrate |
| FeF3 | Iron (III) Fluoride |
| Which process is active when rain forms in the atmosphere? | Condensation |
| CO2 | 6+8+8=22 Protons |
| N2O5 | dinitrogen pentoxide |
| PCl3 | phosphorous trichloride |
| How many sig figs? 0.012 72,700 9.909*10^5 | 2 3 4 |
| NOT capable of forming hydrogen bonds? | CH4 |
| ______will always cause the pressure exerted by a gas to increase | increase in temperature |
| Ca3N2 | Calcium and nitrogen ionic compound |
| chlorine =forms a (-) ion, and is in period 3, group 17 | Cl |
| will NOT speed up a chemical reaction? | catalyst |
| Gold & Silver are in the same_______? | group |
| Argon & Aluminum are in the same______? | period |
| Two 50mg tabs would supply a toxic dose for a patient of 175lb (toxic dose 2mg per kg of body weight)? T/F | False |
| Nitrogen has _______ valance electrons in its outer shell | 5 |
| Fluorine has ______ valance electrons | 7 |
| Atom A and B Isotopes have the same _______ number but different _______ numbers. Are known as isotopes. | atomic number, mass number |
| Molecular compounds | PCl3 Cl2 |
| Because of _________, C8H18 would have the highest boiling point of the following C2H6, C4H10, C6H14, C8H18 | London forces |
| A kicker capable of a kick 55yds should be capable of a kick 55m? T/F | False 55yds =50m |
| It is difficult to breathe in high mountains because the atmospheric pressure is lower therefore there are fewer oxygen molecules to breath. T/F | True |
| One molecule of Fe2(CO3)3 has a mass of ______g? | 291.6g |
| For the following reaction, both adding MgCl2 and lowering the temp will cause a shift to the left. Mg(s) + 2HCl(aq) <------>MgCl2(aq) + heat T/F | False NOT lowering temp |
| ________compounds result from atoms gaining and losing electrons, while ________compounds result from atoms sharing electrons | Ionic molecular |
| As air _________ falls so does air __________ | temperature pressure |
| Since the electronegativity of C is 2.5, and O is 3.5 (True!) chemical bond formed is _________ | polar |
| a double bond results from ___ bonding atoms sharing ___ electrons | 2 4 |
| C(s) = O2(g) ---> CO2(g) heat | Combination exothermic |
| dead chemist | Barium |
| ionic compound NaCl structure | each ion is surrounded by 6 ions of opposite charge in an extended array of ions |
| CO3^2- | carbonate |
| NO3+ | A nitrate dioxaziridin-3-ium 3-oxide |
| MnCl3 | Manganese (III) |
| Cu2SO4 | Copper (I) |
| An element in group 2 can NOT form an ionic bond with ______ | Ca |
| NaNO3 | Sodium nitrate |
| Li, Na, K | all have the same charge when they form ions |
| Elements in group ____ form +1 ions, group ____ form +2, group ___ form -1 ions | 1, 2, 17 |
| Na2SO4 | sodium sulfate |
| Cr3(PO4)2 | chromium (II) phosphate |
| CaCl2 | calcium chloride |
| CoO | Cobalt (II) oxide |
| Ions will lose or gain electrons in order to obtain 8 in their outer shells | Octet rule |
| Cu3N2 | Copper(II)Nitride |
| Ca(OH)2 | Calcium hydroxide |
| If an atom gains one or more electrons it becomes a positive ion. T/F | False |
| K2SO4 | potassium sulfate |
| Cr(NO3)3 | chromium nitrate |
| CrN | chromium nitride |
| Na and F form ____ bonds | ionic |
| Lewis dot for Ca____, N____, Cl____ | 2,5,7 electrons |
| compound formed magnesium ions and carbonate ions | MgCO3 (charge on Mg ion is +2 and charge on carbonate ion is -2) |
| valence electrons group 2 ____ and group 16____ | 2, 6 |
| Mg and P combine to form ionic compound | Mg3P2 |
| FeO | iron (II)oxide |
| Iron (II) is Fe+2 and O forms -2 ions, so FeO Iron (II)- Fe has +2 ion and O has -2 ion forming an ionic bond due to ___ ___ ___ ____. | attraction between opposite charges |
| group 15 ionic charge | 3+ or 5+ |
| Fe2S3 | iron (III) sulfide |
| K2SO4 | potassium sulfate |
| ionic compound of K and N | K3N potassium nitride |
| Na2S charge | +1 |
| ________are used in the chemical formulas of an ionic compound to show how many ions of each type are required for the compound to be neutrally charged. | Subscripts |
| group 17 ______ one electron to form charge of -1. | gain |
| NH4NO3 contains both negative and positive polyatomic ions. T/F | True |
| V(NO3)3 | Vanadium (III) nitrate |
| CaBr2 | Calcium bromide |
| the charge on the Fe ion in FeCl3 is ____ | +3 |
| MgSo4 | magnisium sulfate |
| CuS2 | Copper (I) Sulfide |
| AlCl3 | aluminum chloride |
| Ni2O3 | Nickel (III) oxide |
| CaCO3 | Calcium carbonate |
| Ti(NO3)2 | Titanium (II) |
| Cu3N | Copper (I) |
| HCO3-1 | bicarbonate |
| AlCl3 | aluminum chloride |
| Ni2O3 | Nickel (III) oxide |
| CaCo3 | calcium carbonate |
| NH4NO3 has _____ and _____ polyatomic ions | positive, negative |
| Ti(NO3)2 | Titanium (II) |
| Cu3N | Copper (I) |
| CaCl2, the subscript 2 indicates | there are twice as many chloride ions as calcium ions |
| group 1 | lose 1 electron to form (+1) charged ions |
| group 15 | gain 3 electrons to form (-3) charged ions |
| ionic bonds result from | electrons transfer reactions, one atom loses 1 or more electron to become positive and another atom gains 1 more electron to become negative |
| Ca3(PO4)2 | calcium phosphate |
| CoP | Cobalt (III) phosphide |
| Fe2S3 | iron (III) sulfide |
| K2SO4 | potassium sulfate |
| MgCO3 | magnesium carbonate magnesium+2 carbonate-2 |
| NO3-1 | nitrate |
| NO2-1 | nitrite |
| group 3 valence electron | 3 |
| group 4 valence electron | 2 to 4 |
| group 5 valence electron | 2 to 5 |
| group 6 valence electron | 2 to 6 |
| group 7 valence electron | 2 to 7 |
| group 8 valence electron | 2 or 3 |
| group 9 valence electron | 2 or 3 |
| group 10 valence electron | 2 or 3 |
| group 11 valence electron | 1 or 2 |
| group 12 valence electron | 2 |
| groups 3-12 | transition metals |
| 1 in | 2.54 cm |
| 1 mile | 1.6 km |
| 1 gal | 3.78 L |
| 1 kg | 2.2 lb |
| What is the formula of the ionic compound formed between an iron (III) ion and the ion formed by Cl? | FeCl3 |
| 38.5 in = ? meters | 0.978 m |
| How many electrons? Be, Cl, Ne | Be 2, Cl 7, Ne 8 |
| True of False Because K is in the same period, but left of Br on the p-table, an atom of K is smaller than an atom of Br | False |
| True of False AB2 describes the chemical formula of an ionic compound that forms between the elements in group 2 and group 16. | False /AB |
| Metals form the (-) ions while nonmetals form the (+) ions. True or False | True |
| True or False According to the rules that govern the naming of ionic compounds, the positive ions are always named first followed by the negative ions. | True |
| True or False In a standard periodic table, elements with similiar chemical properties are usually found in the same group. | True |
| Write chemical formulas and the name the compounds for all ionic compounds that would form between the following ions. i.e. Na+ and Cl is NaCl, sodium chloride. K+, Co+3, S-2, NO3-1 | K2S, KNO3, CO2S3, CO(NO3)3 |
| A solution is made by dissolving 75 g of sugar in 450 g of water. What is the % (m/m) of this solution? | [75 g / (75 g + 450 g )] x 100 = 14% (m/m) |
| 26.5 g of NaCl is dissolved in enough water to make 375 mL of solution. What is the % (m/v) of this solution? | (26.5 g / 375 mL) x 100 = 7.07% (m/v) |
| When 37.5 mL of ethanol is mixed with 125 mL of water, the resulting solution has a volume of 159.7 mL. What is the % (v/v) of the ethanol this solution? | (37.5 mL / 159.7 mL) x 100 = 23.5% (v/v) |
| How many g of CaCl2 are in 2.75 L of a 4.80% (m/v) CaCl2 solution? | 4.80% = 0.0480 as a decimal, 0.0480 x 2750 mL = 132 g (4.80 g / 100 mL) = (? g / 2750 mL) ? = 132 g |
| If a particular brand of red wine is 12.5% (v/v) in ethanol, how many mL of ethanol are in a 0.75 L bottle of that red wine? | 12.5% = .0125 as a decimal, 0.125 x 750 mL = 94 mL (12.5 mL / 100 mL) = (? mL / 750 mL) ? = 94 mL |
| What is the mass, in g and mg, of the dissolved O2 in 1.0 kg of water if the level of the dissolved O2 is 0.00080% (m/m)? | (0.00080 g / 100 g) = (? g / 1000 g) ? = 0.0080 g = 8.0 mg |
| One serving (one 12 ounce can = 355 mL) of a soft drink contains 39 g of sugar. How much sugar does a person consume if they drink an entire 2.0 L bottle of the soda? | (39 g / 355 mL) x 100 = 11% (m/v) 11 % = 0.11 as a decimal, 0.11 x 2000 mL = 220 g |
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graftngrl
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