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