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Review for Chemistry Semester 1 Final Exam Cp

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Semester I CP Chemistry Review

Semester I CP Chemistry Review. 2009/2010. 1. What has to happen for a hypothesis to become a theory?. Information technology has to be supported by many, many experiments. ii. Compare the size and mass of the nucleus in an cantlet. (where is virtually of the mass of an atom found?).

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Semester I CP Chemistry Review

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  1. Semester I CP Chemistry Review 2009/2010

  2. one. What has to happen for a hypothesis to get a theory? • It has to be supported by many, many experiments.

  3. 2. Compare the size and mass of the nucleus in an atom. (where is well-nigh of the mass of an atom plant?) • The atom is mostly empty space. Although the nucleus occupies only a minor part of the atom'south volume it contains about of its mass.

  4. 3. All atoms of the same chemical element have the same number of what subatomic particle? • Protons

  5. iv. What subatomic particles are in the nucleus and outside the nucleus? • In nucleus = protons + neutrons • Orbiting around nucleus = electrons

  6. 5a. 131I undergoes beta (β )emission • 13153I  13154Xe + 0-1β (a loss of a beta particle = a proceeds of 1 in atomic # and a no change in mass)

  7. 5b. 230Th undergoes alpha(α) emission • 23090Th  22688Ra + 42α • 42α aka 42He • A loss of 4 atomic mass and a loss of 2 in diminutive #

  8. 5c. 23090Th undergoes gamma emission • 23090Th  23090Th + gamma • No modify but release of energy

  9. 6. Put the three types of decay (alpha, beta, gamma) in order from biggest to smallest. Then circle the type of decay that is the easiest to block. • Alpha particles are the biggest and gamma the smallest • Alpha easiest to block, gamma harder to block • Alpha low energy and gamma high energy

  10. vii. What are alpha particles? Beta particles? Gamma particles? • Alpha are helium nuclei • Beta are electrons • Gamma are photons

  11. 8. What occurs in a fusion reaction? What occurs in a fission reaction? Give an example of each. • Fusion – ii smaller nuclei combine to make one larger nucleus • Fission – One large nucleus breaks down into 2 or + smaller nuclei

  12. 9. How does the free energy produced in a fission or fusion reactions compare to the energy produced in a chemic reaction? • Both fission and fusion release A LOT more energy than a chemical reaction.

  13. eighteen. What is the forcefulness that holds the nucleus together chosen? • Strong nuclear forces 19. What is an isotope? • Atoms with the same # of protons but different # of neutrons.

  14. 20. How do you know if an isotope of an element is radioactive or stable? (recollect there is ratio, 1 for elements #20 and under and ane for those larger than #21) • For elements #20 > the ratio of protons to neutrons is 1:1, then stable • For elements #21 < the ratio of protons to neutrons is 1:i.5, then stable • Or if in band of stability on graph (dots part)

  15. 20.b Describe how an atom of Li would exist changed for each of the following situations: • a. Li cantlet loses or gains a neutron – loses or gains atomic mass • b. Li atom loses or gains an electron – loses becomes a + ion, gains becomes a – ion. • c. Li atom loses or gains a proton – becomes a different element

  16. 22. Place the chemical element from the given electron configuration • 1s2 2s2 2p6 3s2 3p5 – add p's = 17 so Cl • 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 – p's = 38, Sr • 1s2 2s2 2p4 – p's = 8, O

  17. 23. Draw the electron dot (Lewis dot) diagram that indicates the number of valance electrons for #22 a, b and c. Cl Sr O

  18. 24. Bromine (Br) commonly has a -1 charge while Potassium (One thousand )has a +1 charge. Explain why this is and how it relates to the noble gas configuration. Why practice ions normally lose or gain ions to accept a noble gas configuration? • Br has 7 valence electrons and would like 8 to accept a total outer orbital only like the noble gases, so it steals 1 electron away from another atom. • K has 1 valence electron and would similar to lose information technology so so information technology would be left with the adjacent lower free energy level which is full, just similar a noble gas. So K likes to requite its 1 valence electron away.

  19. 25. Indicate which element has the greater diminutive radius and requite a reason for your choice. • a. Na or Li - Na considering atomic radius increases as you lot go downward the group, plus Na has three energy levels and Li only has 2. • b. Sr or Mg – Sr. Sr has 5 free energy levels and Mg but has 3. • c. C or Ge – Ge has 4 energy levels, C has ii • d. Se or O – Se has iv energy levels, O has two

  20. 32. What is the departure between a group and a period on the periodic table? • A group is a column and all in a group accept the same # of valence electrons and comport similarly in a chemical reaction. • A menses is a row and tells you how many free energy levels the element has.

  21. 33. What is electronegativity and what is its tendency downward a grouping and across a row in the periodic tabular array? • The ability of an atom to attract electrons to itself. • F has highest, Fr lowest • Increases from left to right. Decreases every bit y'all get downwards a group.

  22. 34. For each of the following pairs which atom/ion will accept the College ionization energy? Explicate. • a. Ca or Ba? - Ca is higher because it has only 4 energy levels then its valence electrons are closer to its nucleus • b. Al or Cl? – Cl, they both have three energy levels but Cl has more protons attracting its electrons

  23. 35. Where are the metals, nonmetals and metalloids on the periodic table? • Metals to the left, below staircase • Nonmetals to the right, in a higher place staircase • Metalloids along the staircase

  24. 36. How many valence electrons does the cantlet have? • a. Na – 1 (it's in grouping IA) • b. N – v (it'south in group VA) • c. Ga - 3 (it's in group IIIA) • d. Mg – 12 (it's in grouping IIA)

  25. 37. What type of elements form ionic bonds ? Draw what happens to the electrons in an ionic bond? Why do the ions in an ionic compound stay together? • Ionic – metallic with nonmetal • Electrons are transferred from metallic to nonmetal • Metallic becomes + and nonmetal becomes –. Opposites attract. Electrostatic forces.

  26. 36. What type of elements form covalent bonds? What are the electrons doing in a covalent bond? • 2 or more than nonmetals • Electrons are being shared between the atoms

  27. 37. Describe what the electrons are doing in a metallic bond. What types of atoms form metallic bonds? • Bounding main of electrons. Valence electrons are floating from one atom to another. • Metallic bonds form merely between metal atoms!!

  28. 38. What blazon of ions to metals form? How about non-metals? • Metals – cations (+ ions) • Nonmetal – anions (- ions) 39. What is a coefficient? • The number before a formula in a chemical equation. Information technology tells you how many atoms or molecules of that substance is involved in the reaction.

  29. 40. Balance the following equations • 2 Al + 2 H3PO4  2AlPO4 + 3 H2 • __P4 + __S8  __ P4S8 • 2 C2H6 + 7 O2  4 CO2 + half-dozen H2O • two AgNO3 + ___K2S  ___Ag2S + 2 KNO3 • ___H2CO3  ____H2O + ____CO2

  30. 40b. Why must chemic equations be balanced? • Considering matter cannot exist created nor destroyed in a chemic reaction. • So the numbers of elements in the reactants must equal the numbers of elements in the products

  31. 41. What is the mass in grams of each of the following: • a. 1 mole of Al = 27 one thousand • b. 0.v moles of S = 16 g • c. one mole of NaOH = 40 thousand (Na = 23 + o = 16 + H = 1) • d. 3 moles of O2 = 32 g (O = xvi x 2) You lot must use the atomic masses from the periodic table

  32. 42. How many moles are in the post-obit: • b. 22 grams of N2O 22g N2O i mole N2O = 0.5 mole 44g N2O • b. 342 grams of Al2(SO4)3 • 342 grand Al2(SO4)3 1 mole Al2(SO4)three = 1 mole 342 thousand Al2(SO4)3 c. 10 grams of Fe2O3 10g Fe2O3 1 mole Fe2O3 = 0.06 mole 160 grand Fe2O3

  33. 43. How many atoms of molecules are in the following? • a. 2 moles of sugar – 1.2 x 10 24 • b. 0.5 moles of H2O – 3.0 ten 10 23 • c. 42 grams of C3H6 42g C3H6 i mole C3H6 vi.0 x 10 24molecules 42 k C3H6 1 mole C3H6 = 6.02 x 10 23

  34. 43b. How many atoms in • a. 32 g of O 32g O 1mole O 6.02 ten 10 23 atoms 16 g O 1 mole O = 1.two x 10 24 atoms • b. 23 g of Na 23g Na 1mole Na 6.02 ten ten 23 atoms 23g Na i moleNa = 6.02 x 10 23 atoms

  35. c. 36 g of C 36g C 1mole C six.02 10 10 23 atoms 12 1000 C 1 mole C = ane.8 x 1024 atoms

  36. 43c. How many atoms in 1 mole of Br? = 6.02 x 1023 atoms How many molecules in ane mole of Fe2O3? = six.02 x 1023 molecules

  37. 44. Calculate the volume of these gases at STP • a. 1.v moles of Neon 1.5 mole Ne 22. 4 50 = 33.6 L 1 mole Ne b. 32 grams of oxygen 32g O 1 mole O 22.4 50 = 44.viii L 16g O 1 mole O

  38. 48. Given the post-obit balanced equation: 2NH3 + 3O2 + 2CH4  2HCN + 6H2O • A. How many moles of HCN are produced from nine moles of O2? 9 mole O2 2 mole HCN = half dozen moles HCN three mole O2

  39. B. How many moles of NH3 are needed to produce 24 moles of H2o? 24 moles Water ii moles NH3 = eight moles Water 4 moles of Water

  40. 49. Given the post-obit balanced equation: SiO2 + 4HF  SiF4 + 2H2O • a. If 5 grams of HF reacts with SiO2, what mass of H2O forms? 5g HF 1 mole HF 2mole H2O 18g H2O 20 g HF 4 mole HF 1 mole Water = two.25 g H2O

  41. b. If 120 grams of SiO2 reacts with excess HF, how many grams of water will form? 120g SiO2 1mole SiO2 2mole Water 18g H2O 60g SiO2 1 mole SiO2 1mole H2O = 72 g Water

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