front 1 What distinguishes the findings of Dalton from the findings of Democritus? | back 1 Dalton proved experimentally that atoms exist whereas Democritus believed in them. |
front 2 List the seven SI base units. | back 2 length - meters (m) time - second (s) amount of substance - mole (mol) electric current - ampere (A) temperature - kelvin (K) Luminous intensity - candela (cd) Mass - kilogram (kg) |
front 3 Name a unit of measure that is smaller than a gram. | back 3 ? |
front 4 How many meters are in a millimeter? | back 4 0.001 m = 1 mm |
front 5 In which phase are the molecules of a sample held rigidly together? | back 5 The solid phase is the phase in which molecules are held rigidly together. |
front 6 The graph represents the heating of water in a pot. At 150 seconds, the water has just reached a boil. If the heat is left on, what will happen to the temperature and volume of water in the pot? (All temperatures in °C.) | back 6 The temp will remain constant and the volume of the water will go down over time. |
front 7 What happens to the volume of a balloon if you put a balloon inside of a vacuum chamber and decrease the pressure around the balloon? | back 7 If the pressure around the balloon decreases then the volume of the balloon will increase. |
front 8 According to Boyle's Law, pressure and volume are inversely proportional. What does this mean will happen to volume as pressure goes up? | back 8 According to Boyle's law, as pressure goes up, volume goes down. |
front 9 What is the relationship between the temperature of a gas and the kinetic energy of the particles of the gas? | back 9 The higher the temperature of the gas, the higher the kinetic energy of the molecules of that gas. |
front 10 What are the basic assumptions of the kinetic molecular theory? | back 10
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front 11 How many protons and electrons does an aluminum ion have? | back 11 protons: 13 electrons: 10 |
front 12 Describe the types of atoms that form a: a. Covalent bond b. Ionic bond c. Metallic bond | back 12 a. covalent: two non metals b. ionic: metal and non metal c. metallic: two metals |
front 13 What family of the periodic table to each of the following belong to? a. K b. Cr c. F d. Kr | back 13 a. alkai metal b. transition metal c. halogen d. noble gas |
front 14 Name the charges that the following atoms will form an ion. a. Na b. Ca c. Al d. P e. S f. Cl | back 14 a. Na+ b. Ca2+ c. Al3+ d. P3- e. S2- f. Cl- |
front 15 What is the formula for the ionic compound formed by calcium ions and chlorate ions? | back 15 Ca(Cl3)2 |
front 16 What is the formula for the ionic compound formed by strontium and bromine? | back 16 Sr Br2 |
front 17 What is the correct name for NH4 PO4 ? | back 17 ammonium phosphate |
front 18 Consistent with iron being a transition metal, the name for FeSO4 should be what? | back 18 iron (II) sulfate |
front 19 the chemical formula for molybdenum(I) phosphate is what? | back 19 Mo3 PO4 |
front 20 Which is the correct name for the compound P2 O3 ? | back 20 diphosphorus trioxide |
front 21 What is the correct formula for dinitrogen tetroxide? | back 21 N2 O4 |
front 22 In this equation, which are the reactant(s)? Sr(s) + O2 (g) → SrO(s) | back 22 reactants: Sr (s) + O2 (g) |
front 23 Which type of reaction can be recognized by the general pattern? A+BX ----> AX+B | back 23 single replacement |
front 24 Which type of reaction is Al + O2 → Al2 O3 ? | back 24 synthesis |
front 25 What are the correct coefficients when this equation is balanced? Sb + O2 → Sb4 O6 | back 25 4 Sb + 3 O2 ---> Sb4O6 |
front 26 Which are the product(s) of this chemical reaction? FeCl3 + NH4 OH → | back 26 FeCl3 + NH4 OH →Fe (OH)3 + 3NH4Cl Fe3+ Cl- NH4+ OH- |
front 27 Which region is referred to as the s-block on the diagram? | back 27 A |
front 28 Which region contains elements with six valence electrons? | back 28 The column with 7 valence electrons isn't labeled |
front 29 What does the modern periodic law state? | back 29 The physical and chemical properties of the elements are periodic functions of their atomic numbers. |
front 30 Which element has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 ? | back 30 Calcium (Ca) |
front 31 which is the correct electron configuration for the element Manganese (Mn)? | back 31 Mn 25 e- 1s2 2s2 2p6 3s2 3p6 4s2 3d5 |
front 32 Which element has the following electron configuration? [Kr]5s 2 4d 10 5p 5 | back 32 iodine (I) |
front 33 keeping in mind that the cutoff in electronegativity difference between a covalent and and ionic bond is 1.67, a. H2 O b. Li2 O | back 33 a. covalent bond types b. ionic bond type |
front 34 What happens to the valence electrons during the formation of an ionic bond? Or a covalent bond? | back 34 In an ionic bond, one or more valence electrons from one atom (the less electronegative one) are tranferred to the other atom (the more electronegative one). |
front 35 Explain the connection between the type of intermolecular force (hydrogen bonding, dipole-diple forces, or London dispersion forces) and the strength of the intermolecular forces. A sample of molecules with which type of force is expected to have the lowest boiling point? Explain your answer. | back 35 Hydrogen bonding strongest higher bp dipole-dipole forces London dispersion forces weakest lowest bp |
front 36 Describe London dispersion forces. | back 36 A nonpolar molecule forms a temporary dipole, which, increases a dipole is a nearby nonpolar molecule. |
front 37 Explain why ice is less dense than water and therefore floats on water. Use a diagram if you want. | back 37 When liquid water freezes to ice, the positive end of the water molecule aligns with the negative end of a neighboring water molecule. Because the water molecule has a bent shape, there are big spaces in ice, making it less dense than water. |
front 38 In the case of kool aid dissolved in water, name the solute, solvent, and solution. | back 38 Solute - powdered kool aid solvent - water solution - kool aid disovled in water |
front 39 List the factors that affect the rate of solution of a solid in a liquid. | back 39
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front 40 As shown in the following graph, the quantity of solute per 100g of water at a temperature of 50°C for NaNO3 will be ________. | back 40 120g solute per 100g of H2O |
front 41 Which has molecules with more kinetic energy, ice or liquid water? | back 41 molecules of liquid water have more kinetic energy than molecules of ice. |
front 42 Is the following reaction endothermic or exothermic? CH4 (g) + 2O2 (g) → CO2 (g) + 2H2 O(g) ΔH= -890.4 KJ | back 42 Because △H is negative, it is exothermic |