Chemistry Final AU
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| Which abbreviation does not represent an SI unit? | L
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| number of significant figures in 0.04050 is? | 4
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| correct scientific notation for the measurement 108.2 cm? | 1.082 x 10 (2)
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| 1 liter is approximate to | 1 pt
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| the equivalent of 22C in kelvins? | 295
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| Kelvin = | C+273
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| Celcius = | (F-32) x (5/9)
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| Farenheit= | C(9/5) + 32
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| the equivalent of 130K in degrees farenheit | -225
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| true or false: protons are positively charged, and lighter than their negatively charged counterparts | false
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| isotope of an element has 12 neutrons and a relative atomic mass of 24 amu. How many protons does it have? | 12
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| Isotopes of an element differ in their numbers of ___? | neutrons
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| which period contains chlorine | 3
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| Stairstep (metalloids) | B, SI, Ge, Sb, Po
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| subshells in order of increasing energy | s p d f
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| What is the electron configuration for zinc (atomic number 30) | 1s2 2s2 2p6 3s2 3p6 3d10 4s2
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| the charge of a ferric ion is | 3+
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| which element in period 3 would form an ion by loosing three electrons | Al
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| formula for a compound between calcium and phosphorus | Ca3P2
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| according to VSEPR theory, the shape of NI3 is | trigonal planar
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| SI for length | m2
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| SI for mass | kg
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| SI for time | s
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| density | m/v
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| proton, neutron, electron | 1+, 0, 1-
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| Atomic Mass= | Protons(mass) + Neutrons (mass)
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| number of protons equal to | number of electrons
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| ide means | no oxygen
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| ate means | add oxygen. 4 oxygens in box, 3 out of box
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| ite means | add oxygen. 3 oxygens in box, 2 out of box
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| formula for potassium carbonate | K2CO2
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| how many bonds do Group V elements need to complete their octests? | three
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| there are _______ lone pairs of electrons in the Lewis structure of N2 | two
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| the number of lone electron pairs in the Lewis structure for H2O is: | two
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| total number of valence electrons available in methane, CH4, is: | eight
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| H20 is what type of molecule | polar covalent
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| Which molecule has a double bond? a. CH4 b. C2H4 c. C3H6 d. C5H12 | C3H6
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| VSEPR theory predicts that nonbonded electron pairs occupy a (greater/lesser) volume of space than a bonded electron pair | greater
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| formula for sodium hydrogen sulfate | NaHSO4
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| molar mass of (NH4)2CO3 is | 96 g/mol
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| how many moles of H2SO4 are there in 43g of H2SO4 | 0.44
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| when we compare 1 mol of atoms of one element with 1 mol of atoms of another element we can say: | they have the same number of atoms
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| how many grams of CuO are needed to produce 150g of copper? | 188g
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| True or false: a redox reaction is one where electrons are gained an lost | true
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| true or false: a dehydrogenation reaction is one in which a compound is oxidized | false
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| consider the combustion reaction of pentane: C5H12 + O2 → CO2 + H20. What is the sum of all the coefficients in the balanced equation? | 20
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| true or false: the gas laws of Charles, Boyle, Gay-Lussac and Avogadro all relate one property of a gas to a second property, while holding two other properties constant | true
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| a sample of gas has a volume of 252 mL at a pressure of 641 torr. What volume will the gas occupy at the same temperature and a pressure of 760 torr? | 212 mL
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| a gas has a pressure of 3.0 atm at 40 C. What is its pressure at 24 C, assuming its volume remains constant? | 2.8 atm
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| Charle’s Law, which variables must remain constant? | pressure and moles of gas
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| What volume does 14.00 g of nitrogen gas occupy at STP? | 11.2 L
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| which secondary force would be expected to hold together the particles of a liquid with a very low boiling point? | london forces
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| True or false: secondary forces are stronger than covalent bonds | false
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| Molecules with large dipole moments are likely to | have higher boiling points than molecules with no dipole moments
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| hydrogen bonds cannot form in molecules with hydrogen bonded to: | hydrogen
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| photosynthesis proceeds according to this unbalanced equation: CO2 + H2O→ C6H12O6 + O2. What mass of CO2 is needed to produce 20.0g of glucose (C6H12O6)? | 29.3g
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| what mass of CaCl2 is produced from 250g of NaCl in the reaction indicated by this unbalanced equation? NaCl + CaF2 → NaF + CaCl2 | 239g
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| chemical formula for cocaine is C17H21NO4. What is the percent carbon in cocaine? | 67.3
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| Analysis of calcium carbide showed its mass composition is 62.5% calcium and 37.5% carbon. What is its empirical formula? | CaC2
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| Calculate the pressure of a gas, in atmospheres, if it supports a 652mm column of mercury | .858 atm
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| true or false: mass, temperature, volume and pressure are the only variables that determine the physical properties of most gases | true
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| solubility of gas in a liquid ______ as temperature decreases | increases
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| which state does matter undergo a large change in volume on heating? | gas
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| sample gas has a volume of 505 mL at a pressure of 705 torr. What volume will the gas occupy at the same temperature and pressure of 755 torr? | 474 mL
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| Calculate the volume of a 3.0L gas sample at 1.00 atm and 0.0C after it is heated to 85C assuming the pressure remains constant | 3.9L
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| melting point is | same as freezing point
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| true or false: secondary forces are stronger than covalent bonds | false
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| nonpolar substances condense mainly through the action of: | london forces
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| True or false: hydrogen-bonding substances do not experience London forces | false
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| True or false: VSEPR theory predicts that the angles between the central nitrogen and the hydrogen atoms in NH3 measures 109.5 | false
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| True or false: VSEPR theory predicts that angles between the central carbon and the oxygen atoms in CO2 measure 180 | true
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| partial charge distribution for HI | 8+ H-I 8-
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| total number of valence electrons available in methane, CH4, is: | eight
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| Which factor does not affect the shape of a molecule? | Nature of the electron transfer between atoms
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| How many moles of H2SO4 are there in 43g of H2SO4? | 0.44
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| pressure _____ when the force stays the same and the area increases | decreases
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| best describes CO2? | Nonpolar covalent molecule
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| How many liters of water must be added to 4L of a 6M HNO3 solution to produce a 2M HNO3 solution? | 8L
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| what is the concentration of a solution containing 10 mol of copper (II) nitrate in 5.0L of solution? | 2.0M
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| What volume of 4.0M NaOH solution is needed to prepare 0.50L of 0.25M NaOH | 0.03L
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| molar mass of Na3PO4 is: | 164 g/mol
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| molar mass of (NH4)2CO3 is | 96 g/mol
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| OIL RIG | oxidation is loss, reduction is gain
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| Gay-Lussac | P/T
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| Boyle | PV
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| Charles | V/T
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| 1atm = | 760 torr
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| STP | 1 mol gas = 22.4 L at STP
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| avogadro | 6.022 x 10(23)
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| diatomics | H, N, O, F, Cl, Br, I
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| London Forces | weakest intermolecular force
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| dipole dipole | intermolecular force between polar molecules
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| hydrogen bonds | strongest intermolecular forces
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| Hydrogen bonds can only happen with H bonded to | N O F
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| Dillution | V1 x M1 = V2 x M2
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| molarity= | moles/liters
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| Reactions that give off heat are called ______ reactions | exothermic
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| Reactions that absorb heat are called ______ reactions | endothermic
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| Which statement best describes the production of a chlorine molecule according to the reaction Cl + Cl → Cl2 + 242 kJ | bond is formed, reaction is exothermic
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| Why does the speed of some chemical reactions increase when the surface area ¬¬of a solid reactant is increased? | change exposes more reactant particles to possible collisions
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| Which statement describes the characteristics of and endothermic reaction? | ΔHrxn is positive, and the reaction products have more energy than the reactants
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| Which statement is true about the reaction A + B → C + D + heat | Which statement is true about the reaction A + B → C + D + heat
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| True or false: A reaction rate increases when the reactant concentrations increases | true
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| True or false: A reaction rate increases when the reactant concentrations increases | false
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| Ozone is destroyed in the upper atmosphere by a series of reactions: | NO
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| True or false: sometimes catalysts are transformed in the course of a reaction | false
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| True or false: many biochemical processes in the body have low activation energies | true
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| system is said to be in a state of dynamic equilibrium when the: | Concentrations of products and reactants stops changing
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| What is the effect of doubling the concentration of SO3 in an equilibrium mixture for this reaction: 2SO2(g) + O2(g) → 2SO3(g) | SO2 increases more than O2
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| The equilibrium constant expression for the following unbalanced reaction: CO(g) + O2(g) → CO2(g) is | K = [CO2]2/[CO]2[O2]
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| Given this reaction equilibrium AgI(s) → Ag+(aq) + I-(aq), addition of Kl(s) to the solution: | Causes the Ag+(aq) concentration to decrease, and the I – (aq) concentration to increase
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| Which of thee compounds is not a strong acid? | H2SO3
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| Which of these is not a strong base? | Al(OH)3
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| 20. To be classified as an acid, a substance must release _____ ions. | H+
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| determine the pH of a solution with [H3O+]= 1.0 x 10(-7) mol/L | 7
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| Which solution is most acidic? | vinegar
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| Which solution is most basic | household ammonia
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| which of these is the weakest acid? | NH4+
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| According to Bonsted-Lowry theory, ____ are proton donors | acids
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| According to Bonsted-Lowry theory, ____ are proton acceptors | bases
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| which of these solutions will red litmus turn blue? | NaOH
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| Calculate the volume of 4.0M NaOH required to neutralize 0.050L of 2.0M HNO3 | 0.025
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| generally equilibrium reactions: | produce mixtures of both reactants and products in a definite proportion
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| Cake mixes often give “high altitude” directions. Why does more water need to be added for high altitude? | the pressure is lower, and the boiling point of water is lower
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| the boiling point of a liquid is ____ as the atmospheric pressure decreases | decreases
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| Which hydrocarbon has the lowest normal boiling point? | C2H6
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| the designation KCl(aq) means KCl is: | the solute in a homogeneous mixture
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| Which substance is most likely to be insoluble in water? | barium sulfate
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| Which compound is most likely to be soluble in water? | sodium hydroxide
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| T/F Most ionic sulfates and bromides are soluble in water | True
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| T/F: the concentration of a solution remains constant regardless of the volume of solution observed | true
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