front 1 what is the chemical name for baking soda? | back 1 Sodium-hydrogen-carbonate |
front 2 what type of chemical is baking soda? | back 2 base |
front 3 what is the chemical name for vinegar? | back 3 [acetic-acid] |
front 4 What type of chemical is vinegar? | back 4 acid |
front 5 a neutralization reaction occurs when... | back 5 an acid reacts with a base to produce water, salt, and sometimes gas. |
front 6 we can determine the percent yield of a reaction by | back 6 dividing the actual yield by the theoretical yield and multiplying by 100 |
front 7 explain what it means when we say the mole ratio of vinegar to baking soda is 1.5:1 | back 7 its means that the solution will contain 1.5 moles of vinegar and 1 mole of baking soda. there are more moles of vinegar and baking soda is the limiting reactant |
front 8 explain what is means when we say that the mole ratio of vinegar to baking soda is 1:1.5 | back 8 it means that the solution will contain one mole of vinegar and 1.5 moles of baking soda. there are more moles of baking soda and vinegar is the limiting reagent |
front 9 if you react 25.25g of Na2CO3 with 50.0mL of 6.0M HCl, answer the following questions. (molar mass of Na2CO3 = 106.00 g/mol & molar mass of NaCl = 58.45 g/mol)
| back 9 a.) Na2CO3 + 2HCl yields 2NaCl + H2O + CO2
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front 10 1.75g of Ag2O is produced when 3.50 g of Ag reacts with excess O2. What is the percent yield?
| back 10 46.54% |
front 11 What is oxidation? | back 11 the loss of electrons |
front 12 What is reduction? | back 12 the gain of electrons |
front 13 The oxidation number of an atom in a molecule or an ion is defined as... | back 13 the charge an atom has or appears to have as determined by the oxidation-reduction rules |
front 14 An oxidation number can also be called... | back 14 an oxidation state |
front 15 The best way to recognize an oxidation-reduction reaction is... | back 15 to see if the oxidation number changes as a result of the chemical reaction |
front 16 What is the oxidation number of Mg(s)? | back 16 0 |
front 17 What is the oxidation number of H2(g)? | back 17 0 |
front 18 The algebraic sum of the oxidation numbers for the atoms of a neutral compound must be... | back 18 0 |
front 19 In a polyatomic ion, the sum of the oxidation number must be equal to... | back 19 the ion charge |
front 20 What is the oxidation number of C in CO? | back 20 +2 |
front 21 What is the oxidation number of C in CO3 2-? | back 21 +4 |
front 22 What is the oxidation state of fluorine when combined with another element? | back 22 -1 |
front 23 The compound Ca(NO3)2 has ______ calcium atom, _______ nitrogen atoms, and ________ oxygen atoms. | back 23 1 calcium, 2 nitrogen, & 6 oxygen |
front 24 In the compound Ca(NO3)2 for each mole of calcium ions there are ______ moles of nitrate ions and the mole ratio of calcium to nitrate ions is _______. | back 24 2 moles
|
front 25 What is a hydrate? | back 25 a compound that has water molecules loosely attached that can be removed by heating. |
front 26 When the aluminum wire was placed in the solution of the copper ions, what was oxidized? | back 26 Al (s) |
front 27 When the aluminum wire was placed in the solution of copper ions, what was reduced? | back 27 Cu 2+ (aq) |
front 28 When the aluminum wire was placed in the solution of copper ions, what was the oxidizing agent? | back 28 Cu 2+ (aq) |
front 29 When the aluminum wire was placed in the solution of copper ions, what was the reducing agent? | back 29 Al (s) |
front 30 Why was an analytical balance used in the aluminum wire experiment? | back 30 because it is more accurate and can generate more sigfigs than the top loading balance |
front 31 How was the top loading balance used in the aluminum wire experiment? | back 31 it was used to place slightly more than 1 gram of the unknown hydrate into the crucible |
front 32 Why was the Buchner funnel used in the aluminum wire experiment? | back 32 it was used to quickly filter the copper out of the solution that was made |
front 33 what is ethanol? | back 33 ethyl alcohol |
front 34 why was ethanol added to the copper during filtering? | back 34 because it helps to dry the filter paper out because it has a lower boiling point than water |
front 35 What is the entire name of 6M HCl | back 35 6 molar of hydrochloric acid |
front 36 How did the temperature of the solution change when the wire was added? | back 36 temp. increased |
front 37 Thermodynamically what type of reaction does an increase in temperature indicate? | back 37 exothermic reaction |
front 38 Titration involves | back 38 the measurement of the exact volume of a solution of known concentration that is required to react with a measured amount of an unknown substance or solution |
front 39 What is a standard solution? | back 39 a solution of known concentration |
front 40 How is a primary solution made? | back 40 from a solid substance by accurately weighing the solid to four or more significant figures on the analytical balance. then the solid is added to a volumetric flask and diluted with distilled water to get a solution of known molarity. |
front 41 A primary solution is made from a liquid by... | back 41 using a volumetric pipet to measure precise amounts of the liquid and then diluting in a volumetric flask |
front 42 Because NaOH absorbs carbon] [dioxide and water from the air, it cannot be weighed accurately. Therefore, it cannot... | back 42 be a primary standard |
front 43 After it has been standardized, the exact molarity of the NaOH is known & it can be... | back 43 used to standardize an unknown acid solution |
front 44 Potassium hydrogen phthalate | back 44 a primary standard that can be used to standardize NaOH solutions |
front 45 How many moles are needed to titrate one mole of KHC8H4O4? | back 45 one |
front 46 Which acid-base indicator will be used in the experiment? | back 46 phenolphthalein |
front 47 What is the color change in the acid-base reaction? | back 47 colorless to pink |
front 48 We end the titration when... | back 48 one drop of the titrant causes the indicator to change color & the color stays for 30 seconds |
front 49 The indicator color change indicates... | back 49 the end point of the titration and tells us the reaction is complete. |
front 50 Know how to standardize HCl | back 50 pg. 83 |
front 51 Why wasn't it necessary to dry the Erlenmeyer flasks between samples in the standardization of HCl experiment? | back 51 you do not have to dry the flask because you are measuring a definite amount of acid into the flask for each trial & your calculations are based on the exact quantity of acid being added to the flask from the syringe. Therefore, the flask can contain distilled water or distilled water can be added without affecting the experiment |
front 52 What mass of KHC8H4O4 would be neutralized by 25.25mL of 0.1034 M NaOH? | back 52 0.5332 g KHC8H4O4 |
front 53 How many mL of 0.1022 M NaOH are needed to neutralize 5.00 mL of a 0.1152M HCl solution? | back 53 5.64mL NaOH |
front 54 Heat is... | back 54 a form of energy called thermal energy which can pass from an object at high temperature to an object at a lower temperature. |
front 55 A calorimeter is... | back 55 a/an insulated container made so that no heat is lost from the container during the experiment |
front 56 Styrofoam cups are used in this experiment because... | back 56 they are good insulators and relatively inexpensive |
front 57 q H2O means... | back 57 the change in temperature of the water |
front 58 C H2O means... | back 58 the specific heat of water |
front 59 m H2O means... | back 59 the mass of water |
front 60 delta t means.... | back 60 the quantity of the heat of the water |
front 61 Specific heat is... | back 61 the amount of heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius |
front 62 amounts of heat are measured in either... | back 62 [joules] or [calories]. |
front 63 the specific heat of water is... | back 63 4.18 joules/g(degrees celsius) |
front 64 the boiling point is... | back 64 when the liquid molecules get enough energy from the added heat that they form vapor |
front 65 Liquid boils when... | back 65 the vapor pressure = the atmospheric pressure |
front 66 what is inside of the bubbles of a boiling liquid? | back 66 the gaseous liquid that is boiling |
front 67 since atmospheric pressure decreases with increasing elevation, the water has a .... | back 67 lower boiling point at higher elevations |
front 68 explain why the temperature of boiling water can be different on different days even if the elevation is the same | back 68 Air pressure changes when different weather fronts move through an area. The fronts cause changes in air pressures (highs and lows). Therefore, the temperature of boiling water can be different on different days even if the elevation is the same |
front 69 enthalpy is... | back 69 the heat flow of reactions at constant pressure |
front 70 if the temperature of the water in the calorimeter increases, then... | back 70 heat has been given off by the reaction mixture |
front 71 If heat is given off by the reaction, then the reaction is _________. Therefore q H2O is ________ & enthalpy is _________. | back 71 exothermic, positive, & negative |
front 72 Using what you learned about specific heat in lab, explain why an empty metal pan on a stove heats much faster than the same pan filled with water. | back 72 an empty metal pan on the stove heats much faster then the same pan filled with water because the metal pan has a much lower specific heat compared to water so it takes less time to heat. |
front 73 Explain why your car overheats if your fan belt breaks | back 73 if your fan belt breaks there is no more air flowing through to cool the liquid that is absorbing the heat from the engine of the car. |
front 74 explain why your car overheats if your radiator has a hole in it | back 74 your car would overheat if your radiator had a hole in it because all of the water would run out of the radiator so there would be no water flowing through the engine to absorb the heat, thus the car would overheat |
front 75 delta t = | back 75 a change in temp. |
front 76 how is delta t calculated? | back 76 by subtracting the final temp. minus that initial temp. |
front 77 what is the chemical name of CaCl2? | back 77 calcium chloride |
front 78 Why is CaCl2 often used in the winter to melt ice? | back 78 because when it is mixed with water (ice) the reaction is exothermic, thus the ice is melted & less dangerous |
front 79 Charles Law states that.... | back 79 at constant pressure the volume of a given gas is directly proportional to its Kelvin temperature |
front 80 The objective of this experiment is to verify Charles Law by finding ... | back 80 the volume occupied by a gas at 2 different temperatures. |
front 81 Charles law is verified if... | back 81 the volume-to-temperature ratios are close to the same number |
front 82 Boyle's Law states that.... | back 82 the volume of a fixed amount of gas at a constant temperature is inversely proportional to the pressure exerted on the gas |
front 83 We will verify Boyle's Law by... | back 83 using a syringe that has a trapped column of gas and apply weights to increase pressure |
front 84 Avogadro's Law states that... | back 84 the volume of a gas at constant temperature and pressure is directly proportional to the quantity of the gas |
front 85 As you put more moles of air into a balloon the volume... | back 85 increases |
front 86 Amonton's Law states... | back 86 at a constant volume and quantity, the Kelvin temperature and pressure of a gas are directly proportional |
front 87 the combination of all the gas laws is the... | back 87 Ideal gas law |
front 88 the equation of the Ideal gas law is | back 88 PV = nRT |
front 89 STP | back 89 standard temperature and pressure |
front 90 STP is defined as... | back 90 0C and 1 atm. |
front 91 Molar volume of an ideal gas at STP is | back 91 22.4 L |
front 92 Two 125mL _________ flasks will be used in the Charle's Law experiment | back 92 Erlenmeyer |
front 93 What 2 types of clamps will be used in the Charles Law experiment? | back 93 Utility and screw clamps. |
front 94 Closing the ______ clamp could cause the flask to _____ as the air expands | back 94 screw ; explode |
front 95 Use the ______ clamp to remove the flask from the ________ water | back 95 utility ; boiling |
front 96 When the flask is submerged in the cooling bath, check to make sure the rubber tubing ______ completely and the end of the tubing stays ______ the surface of the water. | back 96 opens ; below |
front 97 The volume of the water in the 250mL graduated cylinder = volume of the _________ = volume of hot ________ | back 97 flask ; air |
front 98 Charles Law is proved if the difference of the k value is less than _____ | back 98 0.050 mL/K |
front 99 The Boyle's Law apparatus that is on your table has a ______ with a trapped column of air and a piece of _______ on top which is where you will put the weights | back 99 syringe ; wood |
front 100 the weights in this experiment are ________ | back 100 bricks |
front 101 since the bricks are too heavy to weigh on the balances in the lab, they have all been ______ and ______ for you. | back 101 numbered & weighed |
front 102 The Boyle's law apparatus is not perfect because there is ________ between the ________ and the ______ of the syringe | back 102 friction between the plunger & sides |
front 103 Write the equation used to calculate % yield | back 103 (actual yield / theoretical yield) X 100 |
front 104 The reaction represented on page 109 is exothermic because... | back 104 ; the products have less energy than the reactants |
front 105 Chemists often use models made of balls and sticks or straws to represent... | back 105 atoms & bonds |
front 106 Models are useful in visualizing the arrangements of atoms & bonds in these structures because... | back 106 molecules & atoms cannot be seen with the human eye |
front 107 The atomic theory states... | back 107 that the chemical & physical properties of a substance are determined by the distribution of valance electrons and by the arrangement of the atoms in the molecule |
front 108 A lewis structure is a... | back 108 two dimensional representation of a molecule or ion that shows the atomic symbols of the elements and dots or lines to represent electrons that are either in bonds or are unshared |
front 109 The first step in drawing a Lewis structure is to... | back 109 determine the number of valance electrons |
front 110 Electronegativity | back 110 the ability of an atom to attract ions to itself |
front 111 What is the most electronegative element? | back 111 [Fluorine |
front 112 If an atom does not obey the octet rule how many valance electrons does it have? | back 112 more than 8 |
front 113 Using the chart on page 121, what is the molecular geometry of a substance with the general formula of AX3E? | back 113 Trigonal Pyramidal |
front 114 The general rule for bond length is... | back 114 that single bonds are the longest, double bonds are shorter, and triple bonds are the shortest of the 3 types |
front 115 when compounds have more than one possible Lewis structure, these structures are called... | back 115 resonance forms |
front 116 formal charge of an atom is defined as... | back 116 the total number of [valance] electrons of that atom minus the number of valance electrons it [owns] in the molecule: it owns [all] its unshared valance electrons and [half] of it’s shared valance electrons. |