Question #1: Wednesday January AGENDA YOYO Practice Test Review. AIM Midterm Review

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1 Wednesday January AIM Midterm Review YOYO Take YOYO sheet and start working on it Take out practice test and note the questions you want to go over today AGENDA YOYO Practice Test Review HOMEWORK Castle Learning due TONIGHT Chemistry Midterm TOMORROW Wednesday 1/16 Question #1: A chemist performs the same tests on two homogenous white crystalline solids, A and B. The results are show in the table below. The results of these test suggests that a. solid A contains only ionic bonds and solid B contains only covalent bonds b. Both solids contain only ionic bonds c. Solid A contains only covalent bonds and solid B contains only ionic bonds d. Both solids contain only covalent bonds Solid A has a high melting point, is soluble, and is a good conductor both of which are characteristics of ionic bonds. Solid B shows a lower melting point and is not a conductor, properties of covalent bonds 1

2 Question #2: The particle diagram below represents a solid sample of silver. Which type of bonding is present when valence electrons move within the sample? a. Hydrogen bonding b. Metallic bonding c. Ionic bonding d. Covalent bonding The diagram show silver (Ag) ions, silver is a metal, and the sea of mobile electrons, part of the definition of metallic bonds Question #3: Which ion has the largest radius? a. F- b. Clc. Brd. I- Anions (negative ions) have a larger radius compared to their atoms because they gain electrons Cations (positive ions) have a smaller radius compared to their atoms because they lose electrons Radius increases down a group (column) think the snowman so I is the farthest one down 2

3 Question #4: Which sample at STP has the same number of molecules as 5 liters of NO 2(g) at STP? a. 5 grams of H 2(g) b. 5 liters of CH 4(g) c. 5 moles of O 2 (g) d. 5 x molecules of CO 2(g) B is correct because it doesn t matter what the gas is, according to Avogadro s hypothesis, the same volume of any gas has the same number of molecules don t believe me, convert the given liters to moles then to molecules! Question #5: Which molecule has a nonpolar covalent bond? Non-polar covalent bonds have B.E.N.D (bond electronegativity difference between 0 and about 0.4. Tip: when asked for non-polar/most non-polar, look for two of the same elements combined to each other the difference will be 0 3

4 Question #6: What is the chemical formula for lead (IV) oxide? a. Pb 4 O b. Pb 2 O c. PbO 4 d. PbO 2 Write the symbol for lead and oxide Pb O Write the charges of both (the IV means Pb has a +4 charge) Pb +4 O -2 Criss cross by bringing the number on top of one element to the subscript of the other one Pb +4 O -2 à Pb 2 O 4 Simplify Pb 2 O 4 à PbO 2 Question #7: Which list of elements contains a metal, metalloid, and a nonmetal? The metalloids are the elements a. Ag, Si, I M/ML/NM 2 that touch the bold line staircase b. S, Cl 2, Ar NM/NM/NM on your period table: B, Si, Ge, As, Sb, Te, Po c. K, Cu, Br 2 M/M/NM d. Ge, As, Ne ML/ML/NM Metals are everything to the left of the staircase Nonmetals are everything to the right of the staircase 4

5 Question #8: Given the incomplete equation representing a reaction 2C 6 H 14 + O 2 à 12CO H 2 O What is the coefficient of O 2 when the equation is completely balanced using the smallest whole-number coefficients? a. 13 b. 14 c. 26 d. 19 Start with C 12 H 24 O - 2 End with C 12 H 24 O = 38 Look at what you start and end with 19 is the only coefficient you can add that give you 38 oxygens in the reactants Question #9: Which formula represents a molecule having a nonpolar covalent bond? Non-polar covalent bonds have B.E.N.D (bond electronegativity difference between 0 and about 0.4. Tip: when asked for non-polar/most non-polar, look for two of the same elements combined to each other the difference will be 0 5

6 Question #10: Given the structural formula for ethyne: What is the total number of electrons shared between carbon atoms? a. 6 b. 2 c. 3 d. 4 Every line represents 1 pair or 2 electrons There are 3 lines between the carbons so that means there are 3 bonds, so 3 pairs of electrons OR 6 total electrons The questions asks for electrons so choice A Sometimes they ask for pairs other times they ask for electrons READ CAREFULLY Question #11: What is the chemical formula for iron (III) oxide? a. Fe 3 O 2 b. FeO c. Fe 3 O d. Fe 2 O 3 Write the symbol for iron and oxide Fe O Write the charges of both (the III means Fe has a +3 charge) Fe +3 O -2 Criss cross by bringing the number on top of one element to the subscript of the other one Fe +3 O -2 à Fe 2 O 3 This cannot be simplified any more 6

7 Question #12: What is the gram-formula mass of (NH 4 ) 3 PO 4? a. 112 g/mol b. 121 g/mol c. 149 g/mol d. 242 g/mol Look at how many of each element you have, and the mass (to the nearest whole number) N H P O (3 x 14) + (12 x 1) + (1 x 31) + (4 x 16) = 149 g/mol Question #13: Given the equation representing a reaction O + O à O 2 Which statement describes the changes that occur as the oxygen molecule is produced? a. Energy is released as bonds are broken b. Energy is absorbed as bonds are broken c. Energy is absorbed as bonds are formed d. Energy is release as bonds are formed BARF Breaking Absorbed Release Formed The question shows a bond FORMING between the 2 oxygens so energy is RELEASED Choice B is a correct statement but does NOT describe the equation in the question 7

8 Question #14: The table below shows the number of protons, neutrons, and electrons in four ions. Which ion has a charge of 2-? a. J = +2 b. A = -2 c. G = +1 d. E = -1 Protons = +1 Neutrons = 0 Electrons = -1 Question #15: The table below shows the number of subatomic particles in atom X and in atom Z. Atom X and Z are isotopes of the element a. Nitrogen b. Carbon c. Aluminum d. Magnesium Isotopes are the same element but with a different mass (a different number of neutrons) The number of protons must remain the same different # of protons, different element # protons = atomic number, 6 protons = Carbon 8

9 Question #16: A solid sample of copper is an excellent conductor of electric current. Which type of chemical bonds are in the sample? a. Metallic bonds b. Nonpolar covalent bonds c. Ionic bonds d. Polar covalent bonds Copper is a metal and the copper atoms bond to each other by metallic bonding The sea of mobile electrons allows for metals to conduct electricity Question #17: Given the unbalanced equation: N 2(g) + H 2(g) à NH 3(g) When the equation is balanced using smallest whole-number coefficients, the ratio of moles of hydrogens consumed to moles of ammonia produced is a. 3:2 b. 1:3 c. 3:1 d. 2:3 Balance the equation 1 N 2 + 3H 2 à 2NH 3 Look at the coefficients for hydrogen (H 2 ) = 3 and ammonia (H 2 ) = 2 H 2 :NH 3 = 3:2 9

10 Question #18: Given the formula. the bond polarity between which two atoms has the greatest degree of polarity? a. H and O = 1.2 b. C and C = 0 c. C and O = 0.8 d. H and C = 0.4 Go to Table S and calculate the electronegativity difference (bigger number smaller number) Carbon = 2.6 Hydrogen = 2.2 Oxygen = 3.4 Question #19: What is the number of electrons in a potassium atom? a. 18 b. 19 c. 20 d. 39 Look at the periodic table and find potassium (K) You see the atomic number to be 19 which means it has 19 protons Atom = neutral # electrons = # protons 19 = 19 10

11 Question #20: When a Mg 2+ ion becomes a Mg atom, the radius increases because the Mg 2+ ion? a. gains 2 protons b. gains 2 electrons c. loses 2 electrons d. loses 2 protons Looking at the Bohr diagrams, you can see that the Mg atom has two additional electrons. The keywords here are that the Mg +2 ion becomes a Mg atom. Check the electron configuration of Mg from your periodic table, it is 2-8-2, the ion s electron configuration is 2-8, the radius increases because it gains two electrons. Question #21: At STP, O 2 (g) and O 3 (g) are two forms of the same element that have? a. Different molecular structures and different properties b. The same molecular structures and the different properties c. The same molecular structure and the same properties d. Different molecular structures and the same properties. The two forms of oxygen, O 2 and O 3 will have different molecular structures, therefore they will have different properties. 11

12 Question #22: What is the correct Lewis electron-dot structure for the compound magnesium? Take out your Periodic table and look at the electron configuration for Mg. It is 2-8-2, Mg will lose 2 valence electrons (outer electrons) to get to an octet! Look at Fluorine s electron configuration, it is 2-7, if it gains 1 outer electron, it will finally have an octet! The only choice that shows Mg losing two electrons is choice C. Question #23: Which Lewis electron-dot diagram is correct for a S 2 ion? Look at the periodic table and find Sulfur s electron configuration Remember electrons are negative gaining electrons means getting more negative on the number line! (+) means losing the negative charge, getting more positive on the number line! Sulfur s electron configuration is 2-8-6, it has 6 valence electrons (outer electrons) The -2 indicates, that Sulfur will gain two electrons to achieve an octet! 12

13 Question #24: Which list of elements is arranged in order of increasing electronegativity? Look up the electronegativity a. F, Cl, Br 4.0, 3.2, 3.0 for all elements on table S b. K, Ca, Sc.8, 1.0, 2.4 Choice B is the only one that shows an upward trend! c. Li, Na, K d. Be, Mg, Ca 1.0,.9,.8 1.6,1.3,1.0 The most electronegative atoms are FON, Fluorine, Oxygen and Nitrogen! The most electronegative atoms are FON, Fluorine, Oxygen and Nitrogen! Question #25: Which statement describes the charge and location of an electron in an atom? a. An electron has a negative charge and is located in the nucleus. b. An electron has a positive charge and is located in the nucleus. c. An electron has a negative chare and is located outside of the nucleus d. An electron has a positive charge and is located outside of the nucleus. Electrons are (-) and are located outside of the nucleus. Protons are (+) and are located in the nucleus. Neutrons have no charge and are also located in the nucleus. 13

14 Question #26: Based on table S, an atom of which element has the strongest attraction for electrons in a chemical bond? a. Oxygen 3.4 Electronegativity is the attraction for electrons! b. Nitrogen Look up the 3.0 electronegativity for all of c. Selenium 2.6 the given choices. The higher the number, the stronger the attraction! d. Chlorine 3.2 Question #27: Which electron configuration represents the electrons in an atom of calcium in an excited state? a b c d Eliminate choices A, B, the electron number does not stay the SAME! Choice D can also be eliminated, it s the SAME configuration on the P.T, calcium s ground state configuration. Look at the periodic table and find Calcium (Ca) Look for a choice that shows an electron jumping an energy shell! ** Note the number of electrons should STAY THE SAME! 14

15 Question #28: When an atom of phosphorus becomes a phosphide ion (P 3 ), the radius Non-metal atoms gain a. decreases electrons and that increases b. increases the radius. c. remains the same Negative means you gain electrons, and if you gain stuff you get bigger Question #29: Which three elements have the most similar chemical properties a) Ar, Kr, Br b) K, Rb, Cs c) O, N, Si d) B, C, N Look at your periodic table, look for elements in the same group( same column). Because elements in the same group have the same number of valence electrons (outer electrons) the bonding electrons!, they will exhibit similar chemical properties. Choice B has elements that all belong to group number 1. 15

16 Question #30: The table below shows the atomic mass and natural abundance of the two naturally occurring isotopes of lithium. ** To change % into decimal, move decimal two times to the left. To calculate average atomic mass (Atomic Mass)(nat. abund as decimal) + (Atomic Mass) (nat. abund as decimal) Question #31: The equation below represents a reaction between propene and hydrogen bromide. Synthesis: A+ Bà AB This reaction is classified as a synthesis reaction, in this reaction, two substances react to produce one substance 16

17 Question #32: Base your answer to the following information found ties. 1. Write down the equation C 6 H 12 O 6 à 2C 2 H 5 OH +2CO 2 2. Write down the given information under the equation, label ethanol x C 6 H 12 O 6 à 2C 2 H 5 OH +2CO grams = x grams. 3. Solve for x, x = 138 grams of ethanol Question #33: Each molecule listed below is formed by sharing electrons between atoms when the atoms within the molecule are bonded together. Molecule A: Cl 2 Molecule B: CCl 4 Molecule C: NH 3 Explain why NH 3 has strong intermolecular forces of attraction than Cl 2? This is because NH 3 has the ability to do hydrogen bonding which is a STRONG INTER MOLECULAR FORCE ** Hydrogen bonding likes to have F.O.N Hydrogen bonds with Fluorine, Oxygen and Nitrogen! 17

18 Question #34: Determine the percent composition by mass of oxygen in the compound C 6 H 12 O 6? Use percent composition formula on table T! % composition= (Part/Whole) X 100 Find the mass of the parts: (number of each element in formula) (mass to whole number) Carbon: (6)(12) Hydrogen: (12)(1) Oxygen: (6)(12) 72 g/mol 12 g/mol 96 g/mol Find the whole: = 180 g/mol Plug into the formula: (the question askes about oxygen) (96/180) x 100 = 53.3% Question #35: Explain, in terms of molecular structure or distribution of charge, why a molecule of methane is nonpolar? Draw the Lewis Dot Diagram of Methane CH 4 Anytime you see molecule, write SNAP S- Symmetric N-Non-polar A-Asymmetric P- Polar Methane is symmetric, the molecule is non-polar. If you forget how to draw methane that is ok the question give you the answer, they just want you to explain it 18

19 Question #36: Given the equation: 2 H 2 (g)+ O 2 (g)à 2H 2 O (g) If 8.0 Moles of O 2 are consumed. What is the the total number of moles of H 2 0 produced? Use dimensional analysis 8.0 Moles of O 2 X 2 moles of H 2 O = 16 Moles of H 2 O 1 mole of O 2 (these coefficients were taken from the reaction) Question #37 The bright line spectra is produced when electrons in the excited state ( high state of energy) move back to their ground state ( low state of energy) 19

20 Question #38: The reaction between Aluminum and aqueous solution of copper (II) sulfate is represented by the unbalanced equation below. Al (s) + CuSO 4(aq) à Al 2 (SO 4 ) 3(aq) + Cu (s) Explain why the equation represents a chemical change? Chemical changes are made when NEW products form! In this reaction new products are being formed Aluminum Sulfate is being produced with copper, these new substances will have different chemical properties. 20

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