Chapter 2: Atoms, Molecules, and Ions
|
|
|
- Edmund Lambert
- 6 years ago
- Views:
Transcription
1 A periodic table is required to work many of the problems in this chapter. 1. In a cathode ray tube A) electrons pass from the anode to the cathode. B) electrons pass from the cathode to the anode. C) protons pass from the anode to the cathode. D) protons pass from the cathode to the anode. Ans: B Category: Medium Section: The scientist who determined the magnitude of the electric charge of the electron was A) John Dalton. D) Henry Moseley. B) Robert Millikan. E) R. Chang. C) J. J. Thomson. Ans: B Category: Easy Section: When J. J. Thomson discovered the electron, what physical property of the electron did he measure? A) its charge, e D) its mass, m B) its charge-to-mass ratio, e/m E) its atomic number, Z C) its temperature, T Ans: B Category: Easy Section: Which of the following scientists developed the nuclear model of the atom? A) John Dalton D) Henry Moseley B) Robert Millikan E) Ernest Rutherford C) J. J. Thomson Ans: E Category: Easy Section: Rutherford's experiment with alpha particle scattering by gold foil established that A) protons are not evenly distributed throughout an atom. B) electrons have a negative charge. C) electrons have a positive charge. D) atoms are made of protons, neutrons, and electrons. E) protons are 1840 times heavier than electrons. Ans: A Category: Medium Section: Atoms of the same element with different mass numbers are called A) ions. B) neutrons. C) allotropes. D) chemical families. E) isotopes. Ans: E Category: Easy Section: 2.3 Page 24
2 7. An atom of the isotope 137 Ba consists of how many protons (p), neutrons (n), and electrons (e)? A) 56 p, 137 n, 56 e D) 56 p, 56 n, 56 e B) 56 p, 81 n, 56 e E) 81 p, 56 n, 81 e C) 137 p, 81 n, 56 e Ans: B Category: Medium Section: Give the number of protons (p), neutrons (n), and electrons (e) in one atom of 238 U. A) 146 p, 92 n, 92 e D) 146 p, 28 n, 146 e B) 92 p, 92 n, 92 e E) 238 p, 146 n, 238 e C) 92 p, 146 n, 92e Ans: C Category: Medium Section: Which of the following are isotopes? A) 14 C and 13 C D) 12 C and 12 CO B) 14 C and 14 N E) 14 N and 14 N2 C) 14 N and 14 N 3- Ans: A Category: Easy Section: Complete the following chart, in order from left to right Isotope Mass Number Protons Neutrons Electrons 14 N A) 14, 7, 7, 7 D) 7, 14, 7, 7 B) 14, 7, 14, 7 E) Some other answer C) 7, 7, 7, 7 Ans: A Category: Medium Section: Complete the following chart, in order from left to right Isotope Mass Number Protons Neutrons Electrons A) 40 Zr, 21 B) 19 K, 40 C) 21 K, 19 D) 40 K, 21 E) 38 Sr, 19 Ans: D Category: Medium Section: Complete the following chart, in order from left to right Isotope Mass Number Protons Neutrons Electrons A) 97 Zr, 97 B) 40 Zr, 57 C) 57 La, 40 D) 97 Bk, 80 E) 80 Hg, 97 Ans: A Category: Medium Section: 2.3 Page 25
3 13. Complete the following chart, in order from left to right Ion Mass Number Protons Neutrons Electrons 40 Ca 2+ A) 40, 20, 20, 20 D) 40, 20, 20, 22 B) 40, 20, 20, 18 E) 20, 40, 20, 22 C) 20, 20, 40, 20 Ans: B Category: Medium Section: Complete the following chart, in order from left to right Ion Mass Number Protons Neutrons Electrons A) 4 He, 2 B) 4 Be, 4 C) 4 Be, 2 D) 4 He, 4 E) 2 H, 2 Ans: A Category: Medium Section: The elements in a column of the periodic table are known as A) metalloids. B) a period. C) noble gases. D) a group. E) nonmetals. Ans: D Category: Easy Section: Which of the following elements is most likely to be a good conductor of electricity? A) N B) S C) He D) Cl E) Fe Ans: E Category: Easy Section: Which of the following elements is chemically similar to magnesium? A) sulfur B) calcium C) iron D) nickel E) potassium Ans: B Category: Easy Section: Which of the following elements is chemically similar to oxygen? A) sulfur B) calcium C) iron D) nickel E) sodium Ans: A Category: Easy Section: Which of the following elements is chemically similar to potassium? A) calcium B) arsenic C) phosphorus D) cerium E) cesium Ans: E Category: Easy Section: An anion is defined as A) a charged atom or group of atoms with a net negative charge. B) a stable atom. C) a group of stable atoms. D) an atom or group of atoms with a net positive charge. Ans: A Category: Easy Section: 2.5 Page 26
4 21. Which one of the following is an ion? A) B 3+ B) NaCl C) He D) 14 C E) none of the above Ans: A Category: Easy Section: Which one of the following elements is most likely to form a 2+ ion? A) calcium B) carbon C) fluorine D) oxygen E) sodium Ans: A Category: Easy Section: Which one of the following elements is most likely to form a 2 ion? A) scandium B) selenium C) silicon D) strontium E) iodine Ans: B Category: Easy Section: A magnesium ion, Mg 2+, has A) 12 protons and 13 electrons. D) 24 protons and 22 electrons. B) 24 protons and 26 electrons. E) 12 protons and 14 electrons. C) 12 protons and 10 electrons. Ans: C Category: Medium Section: An aluminum ion, Al 3+, has: A) 13 protons and 13 electrons D) 13 protons and 10 electrons B) 27 protons and 24 electrons E) 10 protons and 13 electrons C) 16 protons and 13 electrons Ans: D Category: Medium Section: An oxide ion, O 2, has: A) 8 protons and 10 electrons D) 8 protons and 7 electrons B) 10 protons and 8 electrons E) 10 protons and 7 electrons C) 8 protons and 9 electrons Ans: A Category: Medium Section: A phosphide ion has: A) 10 protons and 13 electrons D) 15 protons and 18 electrons B) 12 protons and 15 electrons E) 18 protons and 21 electrons C) 15 protons and 15 electrons Ans: D Category: Medium Section: An iron(ii) ion has: A) 24 electrons and a charge of 2+ D) 28 electrons and a charge of 2+ B) 24 electrons and a charge of 2 E) 28 electrons and a charge of 2 C) 26 electrons and a charge of 2+ Ans: A Category: Medium Section: How many protons and electrons are present in one Br ion? A) 35 p, 35 e B) 80 p, 81 e C) 35 p, 34 e D) 35 p, 36 e E) 80 p, 34 e Ans: D Category: Medium Section: 2.5 Page 27
5 30. What are the two different ions present in the compound CaS? A) Ca +, S - B) Ca 2-, S 2+ C) Ca -, S + D) Ca 2+, S 2- E) Ca, S Ans: D Category: Medium Section: What are the two different ions present in the compound Na2S? A) Na2 +, S 2- B) Na +, S 2- C) Na 2+, S 2- D) Na +, S - E) Na 2+, S - Ans: B Category: Medium Section: What are the two different ions present in the compound Li3N? A) Li +, N 3- B) Li3 +, N - C) Li3 3+, N 3- D) Li +, N - E) Li 3+, N 3- Ans: A Category: Medium Section: What are the two different ions present in the compound FeCl3? A) Fe 2+, Cl3 - B) Fe 3+, Cl 3- C) Fe +, Cl - D) Fe 3+, Cl - E) Fe +, Cl - Ans: D Category: Medium Section: What are the ions present in the compound CO2? A) C 4+, 2 O 2- B) C 2+, 2 O - C) C 2+, O 2- D) C 2+, O2 2- E) no ions present Ans: E Category: Medium Section: What are the ions present in the compound CH4? A) C 4+, H + B) C 4-, H + C) C -, H + D) C 4- H 4+ E) no ions present Ans: E Category: Medium Section: Which of the following is an example of an empirical formula? A) C9H12 B) C9H18Cl2 C) C6H6 D) N2O4 E) C2H2O2 Ans: B Category: Medium Section: What is the empirical formula for C10H22O2? A) C10H22O2 B) C5H11O C) C20H44O4 D) C2H11O E) C5H11O2 Ans: B Category: Medium Section: What is the empirical formula for C6H14O? A) C6H14O B) C3H7O C) C2H7O D) C12H28O2 E) CHO Ans: A Category: Medium Section: What is the ion ClO4 named? A) chloride ion D) perchlorite ion B) chlorite ion E) perchlorate ion C) hypochlorite ion Ans: E 40. What is the formula for the ionic compound containing calcium ions and nitrate ions? A) Ca3N2 B) Ca(NO3)2 C) Ca2NO3 D) Ca2NO2 E) CaNO3 Ans: B Page 28
6 41. What is the formula for the ionic compound containing calcium ions and oxide ions? A) CaO B) Ca2O C) CaO2 D) Ca3O E) CaO3 Ans: A 42. What is the formula for the ionic compound containing iron (III) ions and iodide ions? A) FeI B) Fe2I C) FeI2 D) FeI3 E) Fe3I Ans: D 43. What is the formula for the ionic compound containing sodium ions and nitride ions? A) NaN B) Na2N C) NNa2 D) Na3N E) NNa3 Ans: D 44. What is the formula for the ionic compound containing barium ions and sulfate ions? A) BaSO4 B) Ba2SO4 C) BaS D) Ba(SO4)2 E) Ba3S2 Ans: A 45. What are the two different ions present in the compound Al(NO3)3? A) Al 3+, (NO3)3 - D) Al 3+, NO3 3- B) Al +, NO3 - E) Al +, (NO3)3 - C) Al 3+, NO3 - Ans: C 46. What are the two different ions present in the compound NH4NO3? A) NH4 -, NO3 + D) NH4 3+, NO 4- B) NH4 +, NO3 - E) NH4 +, NO 3- C) N 3-, H +, O 2- Ans: B 47. Which is the correct formula for iron(ii) phosphate? A) Fe2PO4 B) Fe3(PO4)2 C) Fe2PO3 D) Fe(PO4)2 E) Fe(PO3)2 Ans: B 48. Which of the following is the formula for hydroiodic acid? A) HIO4 B) HIO3 C) HIO2 D) HIO E) HI Ans: E 49. The formula for calcium phosphate is A) CaPO4. B) Ca3(PO4)2. C) Ca2(PO4)3. D) Ca3P2. E) Ca3(PO3)2. Ans: B 50. The formula for magnesium sulfate is A) MnS B) MgS C) MnSO3 D) MgSO4 E) MgSO3 Ans: D Page 29
7 51. The formula for sodium sulfide is A) NaS. B) K2S. C) NaS2. D) Na2S. E) SeS. Ans: D 52. The name for NH4NO3 is A) ammonium nitrate. D) hydrogen nitrogen oxide. B) ammonium nitrogen trioxide. E) hydrogen nitrate. C) ammonia nitrogen oxide. Ans: A 53. The name for Ba(OH)2 is A) barium hydrogen oxide. D) beryllium hydroxide. B) boron hydroxide. E) barium hydroxide. C) barium hydrate. Ans: E 54. The name for KHCO3 is A) calcium bicarbonate. D) calcium hydrogen carbon trioxide. B) calcium carbonate. E) potassium hydrogen carbonate. C) potassium carbonate. Ans: E 55. The name for CuSO4 5H2O is A) copper sulfate acid. D) copper(ii) sulfate pentahydrate. B) copper sulfate pentahydrate. E) copper(v) sulfate hydrate. C) copper(ii) sulfate acid. Ans: D 56. Give the formula for cobalt(ii) chlorate dihydrate A) CoCl2 2H2O D) Co(ClO3)2 2H2O B) CoClO3(H2O)2 E) Co2(ClO3)3 2H2O C) Co(ClO3)2(H2O)2 Ans: D 57. Name the compound Co(NO3)2 A) Cobalt (I) nitrate D) Cobalt nitrite B) Cobalt (II) nitrate E) Cobalt (II) nitride C) Cobalt (I) nitride Ans: B 58. Name the compound CuSO4 A) Copper (I) sulfate D) Copper (II) sulfate B) Copper (I) sulfite E) Copper (IV) sulfate C) Copper (II) sulfite Ans: D Page 30
8 59. Name the compound Al2O3 A) Aluminum oxide D) Aluminum trioxide B) Aluminum (II) oxide E) Aluminum (I) oxide C) Dialuminum trioxide Ans: A 60. Which is the formula for lead(iv) chloride? A) Pb4Cl B) PbCl2 C) PbCl3 D) PbCl4 E) Pb2Cl4 Ans: D 61. What type of compound is Mg(NO3)2? A) Ionic B) Molecular C) Acid D) Base E) Hydrate Ans: A 62. What type of compound is NH4NO3 A) Ionic B) Molecular C) Acid D) Base E) Hydrate Ans: A 63. What type of compound is IF5? A) Ionic B) Molecular C) Acid D) Base E) Hydrate Ans: B 64. What type of compound is HBrO2? A) Ionic B) Binary C) Acid D) Base E) Hydrate Ans: C 65. What type of compound is NaOH? A) Binary B) Molecular C) Acid D) Base E) Hydrate Ans: D 66. What type of compound is H2SO3? A) Ionic B) Binary C) Acid D) Base E) Hydrate Ans: C 67. What type of compound is NH3? A) Ionic B) Ternary C) Acid D) Base E) Hydrate Ans: D 68. Name the acid H3PO4 (dissolved in water). A) Phosphoric acid D) Hydrophosphate acid B) Phosphorous acid E) Hydrophosphoric acid C) Hydrogen phosphate acid Ans: A Page 31
9 69. Name the acid H2SO3 (dissolved in water). A) Sulfuric acid D) Persulfuric acid B) Sulfurous acid E) Hyposulfurous acid C) Hydrosulfuric acid Ans: B 70. The chemical formula for iron(ii) nitrate is A) Fe2(NO3)3 B) Ir(NO2)2 C) Fe2N3 D) Fe(NO3)2 E) Fe(NO2)2 Ans: D 71. Name the compound Co2(SO3)3. A) cobalt sulfate D) cobalt(iii) sulfite B) cobalt(ii) sulfite E) cobalt(iii) sulfate C) cobalt(ii) sulfate Ans: D 72. Name the compound CrO3. A) chromium oxide D) chromium(iii) oxide B) chromium(ii) oxide E) chromium(vi) oxide C) chromium(iii) trioxide Ans: E 73. Name the compound Cl2O5 A) chlorine pentoxide D) chloride oxide B) dichlorine pentoxygen E) dichloride pentoxide C) dichlorine pentoxide Ans: C 74. Name the compound N2O4 A) nitrous oxide D) dinitrogen tetroxide B) dinitrogen pentoxide E) nitrogen tetroxide C) nitrogen oxide Ans: D 75. Name the compound NO2 A) mononitrogen dioxygen D) nitrogen oxide B) nitrogen dioxide E) nitrite C) dinitrogen monoxide Ans: B 76. Name the compounds SO3 A) sulfur trioxide B) sulfate C) sulfite D) sulfur trioxygen E) sulfur oxide Ans: A Page 32
10 77. The straight chain hydrocarbon that contains six carbon atoms is A) propane B) butane C) pentane D) hexane E) heptane Ans: D Category: Medium Section: What is the law of conservation of mass? Ans: Matter can be neither created nor destroyed. Category: Easy Section: Describe the contributions of Marie Curie. Ans: (note that answers will vary) Marie Curie discovered two new elements, and is one of three people to win two Nobel Prizes. She also suggested the term radioactivity to describe the spontaneous emission of particles and/or radiation. Category: Easy Section: What are the three types of radiation that can be produced by the decay of radioactive substances like uranium? Ans: Alpha, beta, and gamma radiation Category: Easy Section: Marie Curie suggested the name radioactivity to describe the spontaneous emission of particles and/or radiation. Ans: True Category: Easy Section: Using a cathode ray tube, J. J. Thomson determined the magnitude of the electric charge on the electron. Ans: False Category: Easy Section: When a beam of alpha particles passes between two electrically charged plates, the beam is deflected toward the positive plate. Ans: False Category: Medium Section: The proton is about 1840 times heavier than the electron. Ans: True Category: Easy Section: How many electrons, protons, and neutrons does an iron-55 atom have? Ans: 26 electrons, 26 protons, and 29 neutrons Category: Medium Section: How many protons are there in one atom of nickel? Ans: 28 Category: Easy Section: How many protons are there in one atom of magnesium? Ans: 12 Category: Easy Section: 2.3 Page 33
11 88. How many protons are there in one atom of xenon? Ans: 54 Category: Easy Section: Almost all the mass of an atom is concentrated in the nucleus. Ans: True Category: Easy Section: The atomic number is equal to the number of protons in the nucleus of each atom of an element. Ans: True Category: Easy Section: The number of neutrons in all atoms of an element is the same. Ans: False Category: Medium Section: How many protons are there in one atom of uranium? Ans: 92 Category: Easy Section: What are isotopes? Ans: Atoms of the same element that have the same atomic number but different mass numbers. Category: Easy Section: The table below describes four atoms. Atom A Atom B Atom C Atom D Number of protons Number of neutrons Number of electrons Which atoms represent the same element? Ans: Atoms A and D represent the same element, and atoms B and C represent the same element. Category: Medium Section: Consider a neutral atom of the following isotope of sulfur: S How many electrons, protons, and neutrons does the atom contain? Ans: 16 electrons, 16 protons, and 18 neutrons Category: Medium Section: 2.3 Page 34
12 96. How many electrons, protons, and neutrons are in a neutral atom of the following isotope of calcium? Ca Ans: 20 electrons, 20 protons, and 24 neutrons Category: Medium Section: How many electrons, protons, and neutrons are in a neutral atom of the following isotope of krypton? Kr Ans: 36 electrons, 36 protons, and 48 neutrons Category: Medium Section: How many electrons, protons, and neutrons are in a neutral atom of the following isotope of gadolinium? Gd Ans: 64 electrons, 64 protons, and 96 neutrons Category: Medium Section: 2.3 Use the following to answer questions : 99. Use the periodic table above to show where the alkali metals are located. Ans: Group 1A or Group 1 Category: Easy Section: Use the periodic table above to show where the alkaline earth metals are located. Ans: Group 2A or Group 2 Category: Easy Section: 2.4 Page 35
13 101. Use the periodic table above to show where the halogen elements are located. Ans: Group 7A or Group 17 Category: Easy Section: Use the periodic table above to show where the noble gases are located. Ans: Group 8A or Group 18 Category: Easy Section: The elements known as the halogens are useful as disinfectants. Name two halogens. Ans: (two of these) fluorine, chlorine, bromine, iodine Category: Easy Section: Define the term molecule. Ans: A molecule is an aggregate of at least two atoms in a definite arrangement held together by chemical forces. Category: Easy Section: What are the seven elements that naturally occur as diatomic molecules? Ans: Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine Category: Medium Section: Define ion. Ans: An ion is an atom or group of atoms that has a net positive or negative charge. Category: Easy Section: A molecule of antifreeze, ethylene glycol, has the formula C2H4(OH)2. How many atoms are there in one molecule of antifreeze? Ans: 10 Category: Easy Section: How many carbon atoms are in one molecule of CH3(CH2)3CH3? Ans: 5 Category: Easy Section: How many hydrogen atoms are in one molecule of CH3(CH2)3CH3? Ans: 12 Category: Easy Section: The formula for isopropyl alcohol is sometimes written as (CH3)2CHOH to better indicate how the atoms are connected. How many hydrogen atoms would be contained in 3 dozen isopropyl alcohol molecules? Ans: 288 Category: Medium Section: 2.5 Page 36
14 111. Define allotrope. Ans: An allotrope is one of the two or more distinct forms of an element. Category: Easy Section: An empirical formula tell us which elements are present in a compound and gives us the simplest, whole-number ratio of the atoms of these elements in the compound. Ans: True Category: Easy Section: Give the formula for potassium oxide. Ans: K2O 114. Give the formula for magnesium chloride. Ans: MgCl Give the formula for carbon disulfide. Ans: CS Give the formula for potassium hydroxide. Ans: KOH 117. Give the formula for nickel(ii) sulfite. Ans: NiSO Name the following binary compound: FeS. Ans: iron(ii) sulfide or ferrous sulfide 119. Name the following binary compound: NaH. Ans: sodium hydride 120. Name the following binary compound: MnCl2. Ans: manganese(ii) chloride or manganous chloride 121. Name the following binary compound: Fe2O3. Ans: iron(iii) oxide (or ferric oxide) Page 37
15 122. Name the following compound: CuCO3. Ans: copper(ii) carbonate or cupric carbonate 123. Name the following compound: K3PO4. Ans: potassium phosphate 124. Name the following compound: Al(NO2)2. Ans: aluminum nitrite 125. Name the following compound: Cl2O7. Ans: dichlorine heptoxide 126. Give the formula of magnesium nitrate. Ans: Mg(NO3) Give the formula of calcium phosphate. Ans: Ca3(PO4) Give the formula of iron(ii) phosphate. Ans: Fe3(PO4) Give the formula of copper(ii) bromide. Ans: CuBr Give the formula of ammonium sulfate. Ans: (NH4)2SO Give the formula of hydrochloric acid. Ans: HCl 132. Give the formula of carbonic acid. Ans: H2CO3 Page 38
16 133. Give the formula of nitrous acid. Ans: HNO Give the formula of sulfuric acid. Ans: H2SO Name the following: HF. Ans: hydrofluoric acid 136. Name the following H3PO3 Ans: phosphorous acid 137. Write the formula of ammonia. Ans: NH Write the formula of lead(ii) chloride. Ans: PbCl Write the formula of calcium carbonate. Ans: CaCO Write the formula of an anion that contains a metal. Ans: CrO4 2- or Cr2O7 2- or MnO Write the formula of a cation that contains a nonmetal. Ans: NH Give an example of an anion that contains a metal and write the name. Ans: chromate or dichromate or permanganate 143. What is the nitride ion, nitrate ion, and nitrite ion, in that order? Ans: N 3-, NO3 -, and NO2 - Page 39
17 144. What is the sulfide ion, sulfate ion, and sulfite ion, in that order? Ans: S 2-, SO4 2-, SO What is the chloride ion, chlorate ion, and perchlorate ion, in that order? Ans: Cl -, ClO3 -, and ClO What is chloric acid, chlorous acid, and hypochlorous acid, in that order? Ans: HClO3, HClO2, HClO 147. What is ammonia and ammonium ion, in that order? Ans: NH3, NH What is the formula for dinitrogen monoxide? Ans: N2O 149. What is the formula for dibromine heptoxide? Ans: Br2O What is the formula for xenon difluoride? Ans: XeF What is the formula for xenon hexafluoride? Ans: XeF What is the formula for the compound hydrogen peroxide Ans: H2O Name the compound CH3CH2OH Ans: Ethanol Category: Medium Section: Name the compound CH3CH2NH2 Ans: Ethylamine Category: Medium Section: 2.8 Page 40
18 155. What is the formula for octane? Ans: C8H18 Category: Medium Section: What is the formula for nonane? Ans: C9H20 Category: Medium Section: 2.8 Page 41
Chapter 02 Atoms, Molecules, and Ions
Chapter 02 Atoms, Molecules, and Ions Multiple Choice Questions 1. In a cathode ray tube A. electrons pass from the anode to the cathode. B. electrons pass from the cathode to the anode. C. protons pass
Chapter 02: Atoms Molecules and Ions
Chapter 02: Atoms Molecules and Ions A periodic table is required to work many of the problems in this chapter. 1. In a cathode ray tube A) electrons pass from the anode to the cathode. B) electrons pass
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Ch. 2 Practice Test Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which formula/name pair is incorrect? 1) A) Fe2(SO4)3 iron(iii) sulfide
Chapter 2 Atoms, Molecules, and Ions
1. What name is given to the concept that different samples of a given compound always contain the same elements in the same mass ratio? A) Ration Law D) Law of Definite Proportions B) Law of Equality
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A certain mass of carbon reacts with 13.6 g of oxygen to form carbon monoxide. grams
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement
Chapter 2: Atoms, Molecules, and Ions
Download full Download Chemical Principles 7th Edition by Zumdahl Test Bank https://digitalcontentmarket.org/download/download-chemical-principles-7th-edition-by-zumdahl-te st-bank Chapter 2: Atoms, Molecules,
Experiment #3: When 2.0 g of sodium hydroxide reacts with 2.2 g carbon dioxide, 4.2 g of baking soda (sodium bicarbonate) is produced.
Name: Dalton s Atomic Theory: (1) Matter is composed of very small units called atoms. Atom is the smallest unit that possesses the chemical property of an element. (2) An element contains only one type
AP Chemistry (1 of 20) AP Chemistry (2 of 20) AP Chemistry (3 of 20) AP Chemistry (4 of 20) AP Chemistry (5 of 20) AP Chemistry (6 of 20)
Ions Ionic Charges of Representative Elements (1 of 20) (2 of 20) Formulas and Names of Common Metal Ions with More than One Common Ionic Charge Some Common Polyatomic Ions (3 of 20) (4 of 20) Naming Monatomic
Chapter 2: Atoms, Molecules, and Ions
Chapter 2: Atoms, Molecules, and Ions 1. According to the law of definite proportions, A) the ratio of the masses of the elements in a compound is always the same. B) it is not possible for the same two
Cations have a positive charge and anions have a negative charge. 3. Complete the following table.
Name Pre-AP Chemistry: Ionic Bonding and Nomenclature Period Homework #1: Ionic Bonding 1. Use Lewis Dot Diagrams to predict the ionic compound formed between each of the following atoms. Use arrows to
H 2 O. Chapter 9 Chemical Names and Formulas
H 2 O Chapter 9 Chemical Names and Formulas Section 9.1 Naming Ions OBJECTIVES: Identify the charges on monatomic ions by using the periodic table, and name the ions. Section 9.1 Naming Ions OBJECTIVES:
Topic 5: The Language of Chemistry
Topic 5: The Language of Chemistry Chemical Formulas & Chemical Compounds (Chapter 7 in Modern Chemistry) A Chemical Formula Recall that a chemical formula indicates the relative number of atoms of each
CHEMA1301 Selected Questions Chapter 2
CHEMA1301 Selected Questions Chapter 2 1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of. A) the law of multiple proportions B) the law of constant composition
Naming Chemical Compounds
Naming Chemical Compounds Naming compounds is an important part of chemistry. Most compounds fall into one of four categories Ionic Compounds, Molecular Compounds, Acids and Bases, and Hydrates Part One:
4. What is the law of constant composition (also known as the law of definite proportion)?
Name: Exercises #1: 1. What is the law of conservation of mass? 2. Show that the results of the following experiments illustrate the law of conservation of mass. Experiment #1: a 5.00-g sample of pure
Unit 2. Atoms, Molecules, and Ions
Unit 2. Atoms, Molecules, and Ions Upon successful completion of this unit, the students should be able to: 2.1 State and be able to apply the Law of Conservation of Mass, Law of Definite Proportions,
Atoms, Molecules, and Ions
Atoms, Molecules, and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small
CHEMISTRY 103 Help Sheet #2 Atoms, Molecules, and Ions (Text: Ch 2: )
CHEMISTRY 103 Help Sheet #2 Atoms, Molecules, and Ions (Text: Ch 2: 2.1-2.8) Do the topics appropriate for your lecture Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc (Resource page) Nuggets:
Atoms, Molecules and Ions
Atoms, Molecules and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small
+ #n; Z = atomic number = #p + C isotopes: 12 6
CHEMISTRY 103 Help Sheet #2 Chapter 2 (Part I); Sections 2.1.8 Do topics appropriate for your lecture Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc (Resource page) Nuggets: Periodic Table;
Chapter 6 Chemical Names and Formulas
Chemistry/ PEP Name: Date: Chapter 6 Chemical Names and Formulas Chapter 6: 1 9, 12, 14 24, 26 28, 31 36, 40, 42, 49, 52, 53, 56, 58, 62, 67 (37 total) 1. Provide the name and symbol of the ion formed
CHAPTER 2. ATOMS, MOLECULES, AND IONS REMEMBER correct in a different color. Questions
CHAPTER 2 ATOMS, MOLECULES, AND IONS REMEMBER correct in a different color Questions 17. A compound will always contain the same numbers (and types) of atoms. A given amount of hydrogen will react only
Naming Inorganic Compounds. common names systematic names
Naming Inorganic Compounds common names systematic names Molecular Common Systematic Formula name name AgCl Lunar caustic Silver chloride H 2 SO 4 Oil of vitriol Sulfuric acid MgSO 4 Epsom salts Magnesium
10/1/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 2. Chemistry: Atoms, Molecules and Ions
General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 2 Chemistry: Atoms, Molecules and Ions 1 The Structure of the Atom Dalton s Atomic Theory (1808) o Compounds
The chemical formulas of most of the elements are simply their elemental symbol:
Chemical Formulas A chemical formula gives the numbers and types of atoms that are found in a substance. When the substance is a discrete molecule, then the chemical formula is also its molecular formula.
Chemical Formulas Types of chemical formulas [X m Y n ]
![Chemical Formulas Types of chemical formulas [X m Y n ]](/thumbs/89/98748683.jpg "Chemical Formulas Types of chemical formulas [X m Y n ]")
1 Chemical Formulas Types of chemical formulas [X m Y n ] Molecular Actual # of atoms of each element Empirical Structural Relative # of atoms of each element Actual # of atoms and the bonds between them
Chemical Nomenclature Chapter 2.5-8
Chemical Nomenclature Chapter 2.5-8 Octet Rule An octet is 8 valence electrons is associated with the stability of the noble gases does not occur with He, which is stable with two valence electrons (duet)
Experiment #4. Chemical Nomenclature
Experiment #4. Chemical Nomenclature Many everyday and historically important chemical compounds have common names. For example, water is the common name for H 2 O, baking soda is the common name for NaHCO
4) A specific isotope of an element is known to have 15 protons and 16 neutrons. Which symbol would properly represent this isotope?
CHM1025 Exam 2 Chapter 4 & 5 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) All of the following statements about different elements are true
Chemical Nomenclature
Chemical Nomenclature! The first names for chemicals were common names: Sugar, quicklime, Epsom salts, milk of magnesia, gypsom, laughing gas Simple, but not practical, the tell us little about the chemicals
Atoms, Molecules and Ions
Atoms, Molecules and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small
CHEMISTRY 1: Chemical Bonding
CHEMISTRY 1: Chemical Bonding Brown, T.L., LeMay, H.E., and B.E. Bursten. Chemistry: The Central Science 8 th Ed. New Jersey: PrenticeHall, 2002. CHEMICAL BONDS The forces that hold atoms or ions together
Chapter 6 Inorganic and Organic Compounds: Names and Formulas
Chapter 6 Inorganic and Organic Compounds: Names and Formulas 6.1 Octet Rule and Ions 1 Octet Rule An octet is 8 valence electrons is associated with the stability of the noble gases does not occur with
CHAPTER 2 ATOMS, MOLECULES, AND IONS
CHAPTER ATOMS, MOLECULES, AND IONS This chapter is a review of first year chemistry concepts and terminology used to describe atoms and molecules, atomic theory, the periodic table, and the naming of compounds.
Naming Compounds. Part One: Naming Ionic Compounds. Identifying Ionic Compounds
Naming Compounds Naming compounds is an important part of chemistry. Most compounds fall in to one of three categories ionic compounds, molecular compounds, or acids. Part One: Naming Ionic Compounds Identifying
Homework #1 Chapter 2 Atoms, Molecules, and Ions
Homework #1 Chapter 2 Atoms, Molecules, and Ions 19. 1 L (Cl 2) + 5 L (F 2) 2 L (?) For gases the volume is proportional to the number of participles. Since it is proportional, we can simplify the problem
Reaction Writing Sheet #1 Key
Reaction Writing Sheet #1 Key Write and balance each of the following reactions and indicate the reaction type(s) present: 1. zinc + sulfur zinc sulfide 8 Zn (s) + S 8 (s) 8 ZnS (s) synthesis 2. potassium
Systematic Naming. Chapter 9. Two Types of Compounds. Two Types of Compounds 2 Ionic Compounds. Two Types of Compounds.
Chapter 9 Naming Compounds Writing Formulas Systematic Naming There are too many compounds to remember the names of them all. Compound is made of two or more elements. Put together atoms. Name should tell
AP CHEMISTRY THINGS TO KNOW
AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not
Nomenclature of inorganic compounds. = naming non carbon (mostly) compounds. Some definitions:
1 Chemistry 047 Inorganic Nomenclature Nomenclature of inorganic compounds = naming non carbon (mostly) compounds Some definitions: Nomenclature = system used by chemists to name and identify compounds
Chapter 5: Nomenclature
Chem 1025 Prof George W.J. Kenney, Jr Introductory Chemistry, Zumdahl Decoste, 6th ed Last Update: 21July09 Chapter 5: Nomenclature These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the
Naming Simple Compounds
Naming Simple Compounds Ionic Compounds Ionic compounds consist of positive and negative ions. have attractions called ionic bonds between positively and negatively charged ions. have high melting and
Chapter 02 - Atoms, Molecules, and Ions
1. According to the law of definite proportions, a. the ratio of the masses of the elements in a compound is always the same. b. it is not possible for the same two elements to form more than one compound.
CHEMICAL FORMULAS - NOMENCLATURE (The Language of Chemistry)
CHEMICAL FORMULAS - NOMENCLATURE (The Language of Chemistry) Systematic chemical names of inorganic compounds were developed by a group of scientists who were part of the International Union of Pure and
Chapter 2: Atoms, Molecules, and Ions
Chapter 2: Atoms, Molecules, and Ions 1. Which of the following pairs of compounds can be used to illustrate the law of multiple proportions? A) NH 4 and NH 4 Cl B) ZnO 2 and ZnCl 2 C) H 2 O and HCl D)
Honors Chemistry - Unit 5 Chapter 7 - Nomenclature
Honors Chemistry - Unit 5 Chapter 7 - Nomenclature Unit 5 Packet - Page 1 of 16 Vocab Due: Quiz(zes): 1) Test Date: UT Quest: 2) VOCABULARY: 1) monatomic ion 2) cation 3) anion 4) binary compound 4) ionic
Atomic Theory of Matter
Chapter 2: Atoms, Molecules, and Ions Learning outcomes: Learn the basic postulates of Dalton s atomic theory. Describe the key experiments that led to the discovery of electrons and the nuclear model
CHEM 1305: Introductory Chemistry
CHEM 1305: Introductory Chemistry Naming Inorganic Compounds From Chapter 6 Textbook Introductory Chemistry: Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Language of Chemistry By
YEAR 9 SCIENCE CHEMISTRY. Name: Teacher:
YEAR 9 SCIENCE CHEMISTRY Name: Teacher: 1 2 Worksheet 1 Matter Question 1 Classifying Matter Classify the following as matter not. Water, Air, Time, Heat, Clock, Salt, Gravity, Sand, Helium, Vacuum, Gold
Nomenclature PO 4. phosphate ion. HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2. acetate ion. Chemistry 1 Honors: Chapter 7: pp
Chemistry 1 Honors: Chapter 7: pp218-258 PO 4 3- phosphate ion Nomenclature HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2 - acetate ion SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts"
Campbell Chemistry Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature
Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature Name: Schedule 9/1 Thurs 9/2 Fri In Class Using Lab Equipment Lab Polyatomic Ion and Elements Quiz Ionic nomenclature Homework (to be
3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin
Do all work on a separate sheet of paper so that you can show your work. Section A: Measurement and Math 1. Convert the following and show your work: a. 200 meters = miles. b. 650 in = meters c. 4 years=
Chapter 9 Study Guide
Name: Class: Date: Chapter 9 Study Guide Matching Match each item with the correct statement below. a. monatomic ion f. cation b. acid g. binary compound c. base h. anion d. law of definite proportions
CHEM 110: Chapter 2 Practice Test Questions
1 CHEM 110: Chapter Practice Test Questions Multiple-Choice 1) A certain mass of carbon reacts with 1.6 g of oxygen to form carbon monoxide. grams of oxygen would react with that same mass of carbon to
Write the name or formula for:
Do Now Date: Tuesday, November 2, 2015 Objective: Name and write formulas for ionic and molecular (covalent) compounds. Write the name or formula for: K 2 SO 4 NaNO 3 Calcium Hydroxide Tuesday, November
Molecules and Compounds
Molecules and Compounds ed. Brad Collins Some images Copyright The McGraw-Hill Companies, Inc. A molecule is an aggregate of two or more atoms in a definite arrangement held together by chemical bonds
Chapter 2. Chapter 2
Chapter 2 Atoms, Molecules, and Ions Chapter 2 Atomic Theory Model for atom and ions that works well for chemistry Molecules Combinations of atoms Ways of representing molecules: formulas and models Names
Chemical Formulas and Chemical Compounds
CHAPTER 7 REVIEW Chemical Formulas and Chemical Compounds SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. c In a Stock system name such as iron(iii) sulfate, the Roman numeral
Chapter 8 Nomenclature
8.1 Names of Atoms Chapter 8 Nomenclature Simple neutral atoms with no charge are named as is: Na is sodium atom, Ne is neon atom Know the names and symbols for elements #1-20 and Ba, Co, I, Cu, Fe, Pb,
Test- Teacher s Use Only Student s Name Question Max Point Number Score Scored Date Duration Grade Instructions
Physical Science Test- Unit Teacher s Use Only Student s Name Date 2016-2017 Academic Year- Term Question Number Max Score Point Scored Duration Grade minutes G Q1 Q2 Q3 Instructions Fill in your student
Chemistry. Test - Unit Q10 Q11 Q12 Q13 Q14 Q15 Q16 Q17. Total. Teacher s Use Only. Student s Name. Max Score. Question Number. Point Scored.
Chemistry Test - Unit Teacher s Use Only Student s Name Date 2016-2017 Academic Year- Term Question Number Max Score Point Scored Duration Grade minutes G Q1 Q2 Q3 Instructions Fill in your student ID
Part 1: Grams, Moles and Particles
GENERAL CHEMISTRY I CHEM 1311.002 (12681) EXAM 2 Monday, June 18, 2012 Name Banner ID Part 1: Grams, Moles and Particles 1. How many lead atoms are present in 4.216 moles of lead? Avogadro s Number is
Chapter 2. Atoms, Molecules, and Ions
Chapter 2 Atoms, Molecules, and Ions Section 2.1 The Early History of Chemistry Early History of Chemistry Greeks were the first to attempt to explain why chemical changes occur. Alchemy dominated for
Chapter 9 Naming Simple Compounds
Chapter 9 Naming Simple Compounds Monatomic Ions Ionic compounds consists of a positive metal ion and a negative nonmetal ion combined in a proportion such that their charges add up to a net charge of
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Ch 5 Molecules & Compounds STUDY SHEET Accelerated Chemistry /100 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) When elements combine to
Honors Chemistry Study Guide: Chemical Nomenclature, Introduction to the Atom (ch 4, sections 1-3) and the Periodic Table (ch 6, sections 1-2)
Honors Chemistry Study Guide: Chemical Nomenclature, Introduction to the Atom (ch 4, sections 1-3) and the Periodic Table (ch 6, sections 1-2) Provide the correct name or formula for each the following.
FORMULAS AND NOMENCLATURE OF IONIC AND COVALENT COMPOUNDS Adapted from McMurry/Fay, section 2.10, p and the 1411 Lab Manual, p
FORMULAS AND NOMENCLATURE OF IONIC AND COVALENT COMPOUNDS Adapted from McMurry/Fay, section 2.10, p. 56-63 and the 1411 Lab Manual, p. 27-31. TYPES OF COMPOUNDS Ionic compounds are compounds composed of
Name: Hour: Unit 2 Periodic Table Nomenclature. Notepack Chapters 5 and 6
Name: Hour: Unit 2 Periodic Table Nomenclature Notepack Chapters 5 and 6 1 Periodic Table & Nomenclature Chapter 5 Part One: Review of Atomic Structure (Pages 107-121) A. Define atom 1. proton - 2. neutron-
2.1 Atomic Theory of Matter
Chapter 2 2.1 Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter re-emerged in the early nineteenth century, championed by John Dalton. Law of Conservation of Mass
Big Idea: Matter & Atoms
Big Idea: Matter & Atoms Naming Ionic Compounds Naming Covalent Compounds Naming Acids Naming Hydrates The cation (positive ion) is written first Takes the same name as the element if only forms one charge
Balancing Equations Notes
. Unit 6 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
Test bank chapter (2)
Test bank chapter (2) Choose the correct answer NOTE: A periodic table is required to work many of the problems in this chapter. 1. Which of these elements is most likely to be a good conductor of electricity?
Chapter 2. Atoms, Molecules, and Ions
Chapter 2 Atoms, Molecules, and Ions The atomic theory Topics The structure of the atom Atomic number, mass number and isotopes The Periodic Table The atomic mass scale and the average atomic mass Molecules
Atoms, Molecules, and Ions (Chapter 2) 1. a. Give the name and symbol for one alkaline earth metal.
Atoms, Molecules, and Ions (Chapter 2) 1. a. Give the name and symbol for one alkaline earth metal. b. Give the name and symbol for one transition metal. c. Give the name and symbol for one noble gas.
Law of Multiple Proportions Elements are composed of small particles,
CHAPTER 2 Atoms, Molecules, and Ions 2.1 Atomic Theory Democritus (5th century BC) suggested that matter was made of small, indivisible particles, atomos John Dalton (1808) formulated modern atomic theory
Chapter 2. Law of Definite Proportions. Law of Definite Proportions. Law of Conservation of Mass 10/7/2011 WATER H 2 O
Chapter 2 Fundamental Chemical Laws (2.2) Dalton s Atomic Theory (2.3) Defining the Atom (2.5) Atomic Structure (2.6) Molecules and Ions (2.7) The Periodic Table (2.8) Nomenclature (2.9) Law of Conservation
Ion formation: Writing formulae and names for ionic compounds. Having fun with nomenclature! element 1 Ca 2 electrons lost. nonmetallic.
Ion formation: Symbol of Change in electrons element 1 Ca 2 electrons lost Formula of ion Name of ion Metallic or nonmetallic 2 F F 1-3 Al 3+ 4 Zn 2 electrons lost 5 O 2-6 Cs 1 electron lost 7 Ba 2+ 8
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Module 2 Practice Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Elements exhibit similar physical and chemical properties. 1) A) on
2. The reaction of carbon monoxide and diiodine pentoxide as represented by the equation
1. The complete combustion of phenylhydrazine, C 6 H 5 NHNH 2, with the oxidizer dinitrogen tetraoxide is shown in the equation C 6 H 5 NHNH 2 + N 2 O 4 CO 2 + H 2 O + N 2 When balanced, the sum of all
Nomenclature. Common Names. Common Names COMPOUNDS FORMED FROM IONS. Binary Ionic Compounds
PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion World of Chemistry: Chapter 4 Nomenclature HC 2 H 3 O 2 Acetic Acid Common Names Common Names A lot of chemicals have common lot of chemicals have common
Test bank for Introductory Chemistry 5th Edition by Tro
Test bank for Introductory Chemistry 5th Edition by Tro Link download full: https://testbankservice.com/download/test-bank-forintroductory-chemistry-5th-edition-by-tro/ Introductory Chemistry, 5e (Tro)
Chapter 2. Atoms, Molecules, and Ions. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 2 John D. Bookstaver St. Charles Community College Cottleville, MO Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter reemerged in
1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation
NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,
Chemistry CRT Study Guide First Quarter
Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry
Balancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
1
Chemistry 1. In the following list, only is not an example of matter. A. planets B. light C. dust D. elemental phosphorus E. table salt 2. What is the physical state in which matter has no specific shape
CHAPTER 7 CHEMICAL FORMULAS AND BONDING
Name Date Period CHAPTER 7 CHEMICAL FORMULAS AND BONDING IONIC COMPOUNDS 1. What are the two types of bonds that will be discussed in this chapter? 2. How do ionic bonds form? 3. What do you call the positive
name formula name formula ammonium Hydrogensulfate (or permanganate MnO 4 bisulfate) HSO 4 cyanide CN cyanate OCN oxalate
Dr. Abel 1 Chemical Nomenclature Summary A. elements 1 through 94 You will be expected to know the names and symbols on the periodic table throughout the semester. Review these using the table in your
AP* Chapter 2. Atoms, Molecules, and Ions. Monday, September 16, 13
AP* Chapter 2 Atoms, Molecules, and Ions AP Learning Objectives LO 1.1 The student can justify the observation that the ratio of the masses of the constituent elements in any pure sample of that compound
SCH4U Chemistry Review: Fundamentals
SCH4U Chemistry Review: Fundamentals Particle Theory of Matter Matter is anything that has mass and takes up space. Anything around us and in the entire universe can be classified as either matter or energy.
Chemistry Chapter 7 Test
Chemistry Chapter 7 Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A chemical formula includes the symbols of the elements in the compound and subscripts
INSTRUCTIONS ON EVERY AP EXAM:
Most Common Reaction Types: 1. Acid-base neutralization (both weak & strong) 2. Nonmetal and metal oxides with water 3. Active metals with water 4. Single replacement redox 5. Double replacement precipitation
CRHS Academic Chemistry Unit 6 - Nomenclature Practice Problems
Name Period CRHS Academic Chemistry Unit 6 - Nomenclature Practice Problems Due Date Assignment On-Time (100) Late (70) 6.1 6.2 6.3 6.4 6.5 6.6 Warm-Up EC Notes, Homework, Exam Reviews and Their KEYS located
Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms,
Chemical Bonding Valence electrons (the outer most electrons) are responsible for the interaction between atoms when forming chemical compounds. Another way to say that is that valence electrons are the
CHEM 1105 S10 January 21, 2014
CHEM 1105 S10 January 21, 2014 Chapter 3: Compounds and Formulas Today: Types of compounds: Ionic vs. covalent Naming ionic compounds Naming binary covalent compounds (two elements only) Ionic Bonding
Voltage source. Voltage source. Voltage source
Chapter 2 Atoms, Molecules, and Ions History Greeks Democritus and Leucippus atomos Aristotle elements Alchemy 1660 Robert Boyle experimental definition of element. Lavoisier Father of modern chemistry
Nomenclature. Naming Compounds
Nomenclature Naming Compounds Ionic Compounds Metal bonding with non-metal One atom gains electrons, one atom loses electrons Exist as ions with full highest energy levels. Are held together in a giant
Due Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment
Due Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment 2017-2018 You will have a quiz on the first day of school (August 16 th, 2017) on the polyatomic
EIT Chemistry Review S01 Dr. Mack Chemistry is really Chem is try Download available at: www.csus.edu/indiv/m/mackj/ Or look for Jeffrey Mack under CSUS faculty web pages Part 1 To do chemistry, you must: