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Quizzes and Exams

Quizzes and Exams. Please write in non-erasable blue or black pen , no pencil! (Will lose 1 point for pencil or erasable ink) I will put periodic table on backs of quizzes, if you need them.

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Quizzes and Exams

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  1. Quizzes and Exams • Please write in non-erasable blue or black pen, no pencil! (Will lose 1 point for pencil or erasable ink) • I will put periodic table on backs of quizzes, if you need them. • BOX answers! If it’s not obvious where (or which) the answer is that I’m supposed to grade, it will get no credit. • Remember to bring your non-programmable calculators to class on Wednesdays. • Make sure your answers make sense (can there be 23 grams of zinc in a 4.75 g sample of zinc oxide?). • You may only use approved calculators on quizzes; others will be confiscated for the duration of the quiz or exam.

  2. Chapter 2: Atoms and Elements • Dalton’s Atomic Theory is based on empirical observations, formulated • as Laws of Conservation of Mass No detectable gain or loss of mass occurs in chemical reactions. Definite Proportions In a compound, elements are always combined in the same proportion by mass. Multiple Proportions Whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers. 2. Summary of Dalton’s Theory • --Matter consists of tiny particles called atoms. • --Atoms are indestructible. In chemical reactions, the atoms rearrange but they do not • themselves break apart. • --In any sample of a pure element, all the atoms are identical in mass and other properties. • --The atoms of different elements differ in mass and other properties. • --In a given compound the constituent atoms are always present in the same fixed • numerical ratio.

  3. Sample Problems 1. A sample of caffeine contains 96.1 g of carbon for every 10.1 g of hydrogen. If another sample of caffeine contains 30.0 g of carbon, how many g of hydrogen does it contain? 2.* Phosphorus forms two compounds with chlorine. In 5.5 g of one of these compounds, there were 1.24 g of P. In 5.5 g of the other compound, there were 0.818 g of P. Explain how these compounds exhibit the law of multiple proportions.

  4. “Modern” View of an Atom electrons(-) form a diffuse cloud around the nucleus ~Where is most of the mass of an atom? Matter is neutral, so # of electrons = # of protons nucleus has protons(+) and neutrons ~If there is a different number of protons, it is a different ___________? ~If there is a different number of neutrons, it is a different __________? Mass proton  neutron  1 amu electron  10-4 amu (amu = 1.66 x 10-24 g = 1/12 of mass of 12C) Atomic number, Z = # of protons Mass number, A = # of protons + number of neutrons Isotopes = atoms of the same element with different mass numbers AE Z

  5. Sample Problems If a beryllium atom has 4 protons, then it should weigh 4 amu; but it actually weighs 9 amu! Where is the extra mass coming from? How many protons, electrons, and neutrons are in an atom of 52Cr? 24

  6. Some Notes on Charge • Two kinds of charge called + and – • Opposite charges attract • + attracted to – • Like charges repel • + repels + • – repels – • To be neutral, something must have no charge or equal amounts of opposite charges

  7. The Periodic Table Decides ordering of elements Average among all isotopes Transition metals Inner transition elements

  8. Types of Elements Metals: Shiny, malleable, ductile solids with high mp and bp Good electrical conductors Nonmetals: Gases, liquids, or low-melting solids Non-conductors of electricity Diatomic elements: H2, O2, N2, F2, Cl2, Br2, I2 Metalloids: Intermediate properties, often semiconductors

  9. Predicting Ionic Charges Noble gases have very favorable electron configurations. The other elements are jealous… If an ion forms, it will commonly match the nearest noble gas. 1A He 2A 3A 5A 6A 7A N? F? Ne Li+1 N-3 O-2 F-1 Mg+2 Na+1 S-2 Cl-1 Al+3 Ar Kr Ca+2 K+1 Se-2 Br-1 Rb? Sr+2 Rb+1 Te-2 I-1 Xe Rn Ba+2 Cs+1

  10. Calculating Atomic Mass (Weighted Avg) Atomic Mass = ∑ (fraction of isotope n) x (mass of isotope n) = (fraction1∙mass1) + (fraction2 ∙ mass2) + (fraction3 ∙ mass3) + … n Example 63Cu has mass = 62.9396, natural abundance 69.17%, and 65Cu has mass = 64.9278 and natural abundance 30.83%. What is the atomic mass? Answer: Atomic mass = (62.9396)(0.6917) + (64.9273)(0.3083) = 63.55 amu (4 sig fig!)

  11. Sample Problems 1. In a class A is worth 4 points and B is worth 3. Out of 20 grades, if you have 4 A’s (20%) and 16 B’s (80%), what is your average? If an element has two isotopes, A (Z = 4 amu) and B (Z = 3 amu), and their natural abundance is 20% A and 80% B, what is the average molecular weight? 2. Naturally occurring boron (Z = 10.8110 amu) is composed of two isotopes, 10B and 11B. Atoms of 10B have a mass of 10.0129 amu and those of 11B have a mass of 11.0093 amu. Calculate the percentages by mass of the individual isotopes, 10B and 11B.

  12. The Mole; How Chemists “Count” 1. Avogadro’s Number -- The Chemists’ “Dozen” N0 = number of atoms in exactly 12 g of carbon-12 = 6.022 x 1023 “things” ( a very large number!) This is a conversion factor, just like 12 things per dozen, e.g. Mass of one atom of carbon-12 = (12.0 g)/6.022 x 1023 atoms) = 1.99 x 10-23 g/atom 2. The Mole One Mole of a substance contains an Avogadro’s number of formula units. e.g. 1 mole of H2O = 6.022 x 1023 H2O molecules

  13. Sample Problems • How many atoms of gallium are there in 0.2398 moles of gallium? • How many molecules of sugar are there in 0.2398 moles of sugar? • How many marbles are there in 0.2398 moles of marbles?

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