+ #n; Z = atomic number = #p + C isotopes: 12 6

Size: px
Start display at page:

Download "+ #n; Z = atomic number = #p + C isotopes: 12 6"

Transcription

1 CHEMISTRY 103 Help Sheet #2 Chapter 2 (Part I); Sections Do topics appropriate for your lecture Prepared by Dr. Tony Jacob (Resource page) Nuggets: Periodic Table; Isotopes; Counting neutrons, protons, electrons; Average Atomic Weight; Ionic versus molecular compounds; Naming chemicals; Writing formulas from names; Polyatomic ions; Coulomb s law EXPERIMENTS o Rutherford's Au Foil Experiment: Mass of atom is concentrated in highly dense nucleus that was positively charged; rest has little mass; later split the atom (Some instructors cover different historical experiments; be familiar with what is covered by your instructor.} ATOMIC STRUCTURE Nucleus: contains nearly all the atom s mass; neutrons and protons located in the nucleus; very small volume of atom; extremely dense; atom is mostly empty space Electron (e - ): has a charge of -1; mass 1 x 10 7 g ( x 10 8 g) Proton (p + ): has a charge of +1; mass 1 x 10 4 g ( x 10 4 g) Neutron (n): has a neutral charge; mass 1 x 10 4 g ( x 10 4 g) Relative masses: n > p + >> e - ; mass of n p + 1 with e - 1/2000 Elements: determined by the number of protons they contain Masses of all atoms are compared to mass of 12 C with 12 C defined as unified atomic mass units (exact value); 12 C is the standard; unified atomic mass units = u; 1 u = 1 / x = x 10 4 grams ISOTOPES: elements with the same #p + (same element) but different #n (different mass) Isotope Symbol: Z A Element Symbol A = mass number = #p + + #n; Z = atomic number = #p + C isotopes: 12 6 C, 13 6 C, and 14 6C; the 3 isotopes of C each have Z = 6 (6p + ) but different #n (6, 7, and 8) H isotopes: 1 1 H = H, 2 1 H = 2 1 D = D, 3 1 H = 3 1 T = T; D = deuterium; T = tritium Abundance: percent of one isotope as compared to all atoms of that given element Average Atomic Mass (sometimes called Atomic Weight; AW): weighted average of all isotopes of one element taking into account the abundance of each isotope (also called weighted average mass); units = u; (e.g., average atomic mass Br = 79.90u) AVERAGE ATOMIC MASS (AAM) = Σ(mass of isotope) x (fractional abundance) AAM = (mass iso1 )(fractional abundance iso1 ) + (mass iso2 )(fractional abundance iso2 ) + = AAM = (M 1 )(FA 1 ) + (M 2 )(FA 2 ) + Sum of fractional abundances = 1 (i.e., 100%); for elements with only 2 isotopes: FA 1 + FA 2 = 1 Example 1: Calculate the average atomic mass of an element given following data: isotope 1: u, 92.21% abundance; isotope 2: u, 4.70% abundance; and isotope 3: u, 3.09% abundance. Answer: AAM = (M 1 )(FA 1 ) + (M 2 )(FA 2 ) + (M 3 )(FA 3 ) = (27.977)(0.9221) + (28.976)(0.0470) + (29.974)(0.0309) = 28.09u Example 2: What are the abundances of the 2 isotopes of B: 10 B (mass = ), 11 B (mass = ), and average atomic mass of B is ? Answer: AAM = (M1)(FA1) + (M2)(FA2); = x y; since there are 2 unknowns 2 equations are needed; second equation: FA1 + FA2 = 1; x + y = 1 y = 1 - x; substitute this into the first equation: = x (1-x); solve for x: = x x = x x = = 19.90%; y = 1-x = = = 80.10%; since x was the abundance for 10 B abundance of 10 B = 19.90% and abundance of 11 B = y = 80.10%}

2 Mass Spectroscopy: a technique that yields a plot (mass spectrum) of mass versus abundance (or intensity) Example: Mg has 3 isotopes: 24 Mg (79% abundance), 25 Mg (10% abundance), 26 Mg (11% abundance). Draw the mass spectrum for this element? Answer: Mg Mass 30 IONIC Compounds: contain metal + nonmetal (can substitute a polyatomic ion for either or both) Properties: extended solids; not molecules; high melting/boiling points; conducts electricity in molten state; Examples: NaCl(s), Ca(NO 3 ) 2 (s), NH 4 NO 3 (s), AgCl(s) Ions: atoms or molecules that have lost/gained e - (charges are not changed by gaining/losing protons!) Cations: positively charged atoms (electrons have been lost) Anions: negatively charged atoms (electrons have been gained) Polyatomic Ions: many-atom ions ; these compounds are not broken up and are treated as a group NH 4 +, NO 3 -, SO4, OH -, PO 4-3, CO 3, HCO 3 -, CH3 COO -, etc. (these often need to be memorized) Ionic Compound Naming Metal + Nonmetal ionic compound; example: What is the name for CaCl 2? Metal name followed by nonmetal root +"ide" Answer: calcium chloride Metal + Polyatomic ion ionic compound; example: What is the name for Ca 3 (PO 4 ) 2? Metal name followed by polyatomic ion name Answer: calcium phosphate Two Polyatomic ions ionic compound; example: What is the name for (NH 4 ) 2 SO 4? Polyatomic ion name followed by polyatomic ion name Answer: ammonium sulfate Transition Metal example: What is the name for Fe 2 (SO 4 ) 3? 1. Transition metals have charges that vary so the metal charge needs to be specified and is written in Roman numerals in parentheses after the metal name 2. Find charge on Fe. First, SO 4 charge is (memorized); 3() = -6 from 3 SO 4 ; since the compound is neutral the 2 Fe must total +6 ea Fe = +3; Fe Metal name (charge in Roman numerals) followed by polyatomic ion name Answer: iron(iii) sulfate Ionic Compound Writing Formulas 1. Take metal name or polyatomic ion and write formula including charge If metal has a Roman numeral, then charge is determined from that numeral (e.g., copper(ii) = Cu +2 ) If it does not have a Roman numeral, it is a memorized polyatomic ion (e.g., ammonium = NH 4 + ) or determined from column Periodic Table it resides in (e.g., magnesium = Mg +2 since it is in column IIA) 2. Take nonmetal name or polyatomic ion and write formula including charge If nonmetal name ends with ide it is a single atom ion with a negative charge with the charge determined from column in Periodic Table it resides in (e.g., chloride = Cl - since column VIIA has a -1 charge); exceptions: hydroxide (OH - ) and cyanide (CN - ) are polyatomic ions even though the name ends in ide If name ends with ite or ate, or starts with hypo or per it is a memorized polyatomic ion 3. Balance charges within formula Example: Write formula for chromium(iii) carbonate Cr +3 from Roman numeral; carbonate = CO 3 (memorized) Cr x (CO 3 ) y ; choose x and y to balance charge: x = 2 [2(+3) = +6] and y = 3 [3() = -6]; +6 balances -6 Cr 2 (CO 3 ) 3 Charges on elements in Ionic Compounds based on the column of Periodic Table the element resides in: Group IA: +1 (H +, Li +,...) Group IIA: +2 (Be +2, Mg +2,...) Group IIIA: +3 (B +3, Al +3,...) Group VA: -3 (N -3, P -3,...) Group VIA: (O, S,...) Group VIIA: -1 (F -, Cl -,...)

3 MOLECULAR Compounds contain 2 nonmetal elements; Examples: CO, CO 2, N 2 O 4 Naming: Prefix (if greater than 1)+1st nonmetal name & Prefix(always)+2nd nonmetal root+"ide Prefixes: mono (1), di (2), tri (3), tetra (4), penta (5), hexa (6), hepta (7), octa (8), nona (9), deca (10) Example: What is the name for NO? (Has 2 nonmetals molecular compound) Has one N no prefix nitrogen; has one O prefix always used = mono; monoxide answer: nitrogen monoxide Example: What is the name for N 2 O? (Has 2 nonmetals molecular compound) Has two N use prefix = di dinitrogen; has one O prefix always used = mono; monoxide answer: dinitrogen monoxide Writing Formulas - translate name with prefixes Example: What is the formula for disulfur trioxide? disulfur 2S; trioxide 3O; answer: S 2 O 3 ACIDS Naming chemicals named as acids are neutral compounds (e.g., SO 4 and HSO 4 are not named as acids but H 2 SO 4 is named as an acid) Acids that contain anions ending in ide : change ide to ic, add hydro in front and acid at end; e.g., Cl - = chloride; HCl = hydrochloric acid ate : change ate to ic and add acid at the end; e.g., SO 4 = sulfate; H 2 SO 4 = sulfuric acid Common acids to know: Strong acids: HCl (hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid), HNO 3 (nitric acid), H 2 SO 4 (sulfuric acid), HClO 4 (perchloric acid); Weak acids: HF (hydrofluoric acid), HCN (hydrocyanic acid), H 3 PO 4 (phosphoric acid), HC 2 H 3 O 2 = CH 3 COOH (acetic acid) (often good to memorize acetic acid), H 2 CO 3 (carbonic acid) Organic Compounds - This material is usually not covered in Chem 103. COULOMB S LAW: Describes the attractive force between a positive (cation) and negative (anion) ion Force of Attraction = k (Q 1 )(Q 2 ) d 2 Q 1, Q 2 are charges on the ions; d is distance between the centers of the nuclei ionic charges (Q) or ionic radii = d Force mp/bp (ionic radii as you go up a column) 1. Determine the number of protons, neutrons, and electrons present in each of the following atoms. a Cr b Mn c. 9 4 Be d Ca e. 3 1 H 2. How many p +, n, and e - are in each of the following ions? a Al +3 b Ca +2 c Ni +2 d Cl 3. Write the complete isotopic symbol with mass and atomic number for each atom: a. a neutral atom with 28 protons and 30 neutrons b. contains 22 protons and 21 neutrons c. an oxygen atom with 10 neutrons d. chromium atom with a mass number of 54 e. a halogen with 35 protons and 44 neutrons f. an alkali metal with the fewest protons and 4 neutrons g. an iron atom with mass number of 56 and 3 more protons than electrons h. sulfide ion with 17 neutrons 4. For each, state whether the statement is true or false? a. The number of neutrons distinguishes carbon from nitrogen. b. Elements are neutral because they have equal numbers of protons and electrons. c. Elements that have different numbers of neutrons are called isotopes. 5. How many p +, n, and e - are in the isotopic sulfate (SO 3 ) ion: 33 S 16 O 18 O 18 O?

4 6. Which of the following statements is false? a. All atoms contain neutrons. b. All atoms contain protons. c. The mass of the neutron is greater than the mass of the proton? d. The electrons form a cloud around the nucleus. e. Atoms can easily gain or lose electrons but can not easily gain or lose neutrons. 7. Thoroughly describe the Rutherford experiment with a diagram. 8. Oxygen exists as three isotopes: 18 8 O, 17 8 O, and 16 8 O. If the average atomic weight of oxygen is , what do you expect the abundance of 18 8 O to be approximately? <5% 25% 50% 75% 90% 9. An element has two naturally occurring isotopes with the following abundances and masses: Isotope Atomic Mass (u) Fractional Abundance What is the average atomic mass of this element? What is the identity of the element? 10. Silver is found commonly as two isotopes: 107 Ag (mass = u) and 109 Ag (mass = u). The average atomic mass of silver is u. What are the percent abundances of the two isotopes, 107 Ag and 109 Ag? 11. There are 2 isotopes of Cl: 35 Cl (mass = u) and 37 Cl (mass = u). If the average atomic mass of Cl is u, what are the percent abundances of the Cl isotopes? 12. There are 3 isotopes of magnesium: 24 Mg (mass = u), 25 Mg (mass = u), and 26 Mg (mass = u). If the abundance of 25 Mg is 10.00% what are the percent abundances of the other two isotopes of magnesium? 73.7% 8.3% 7.4% 5.4% 5.2% 13. Shown is the mass spectrum of Ti. What is the average atomic mass of Ti? m/e Chlorine, Cl 2, exists as a diatomic gas. During a mass spectrometer experiment a sample of chlorine was analyzed. Chlorine is found as a two isotopes: 35 Cl and 37 Cl with approximate abundances: 35 Cl = 75% and 37 Cl = 25%. a. Draw a mass spectrum that would be expected for atomic chlorine (i.e., for Cl). Include on the x-axis mass values and on the y-axis the peak intensity. Assume the isotopic mass number is the mass of that isotope (i.e., 35 Cl has a mass of 35). b. How many peaks are expected in the mass spectrum for Cl 2? c. What would be the mass and intensity of each peak in the mass spectrum for Cl 2? d. Draw the expected mass spectrum for Cl 2.

5 15. a. Which of the following elements are metals? Ar, Mn, C, O 2, Al b. What is the name of the family of elements that contains magnesium? c. Name one halogen element. 16. Which of the following will have the highest melting point? a. BeO b. NH 3 c. MgS d. KBr 17. Which of the following compounds would have properties most similar to CaF 2? a. CO 2 b. SF 2 c. MgCl 2 d. NaCl e. CaO 18. Name the following molecules. a. NO b. PCl 3 c. KBr d. Na 2 CO 3 e. N 2 O 4 f. K 2 SO 4 g. Ca 3 (PO 4 ) 2 h. Cu 2 O i. Mn 3 (PO 4 ) 2 j. Co(CH 3 COO) 3 k. CoSO 4 l. KMnO 4 m. CH Write the chemical formula for the following names. a. sulfur trioxide b. calcium fluoride c. chlorine monobromide d. sodium sulfate e. ammonium nitrate f. lithium carbonate g. calcium nitrate h. manganese(iii) sulfate i. chromium(vi) oxide j. titanium(iv) sulfide 20. Which of the following when placed in an ionic compound, will commonly have a charge of 2? I. Cl II. O III. SO 4 IV. Ca V. PO 4 VI. NO 3 a. II b. II and III c. II and IV d. II, III, and IV e. II and VI (see Practice Sheet #3 for polyatomic ion naming/writing formula practice; see Practice Sheet #4 for practice naming and writing formulas of compounds) ANSWERS 1. a. 24 p +, 24 e -, 29 n b. 25 p +, 25 e -, 30 n c. 4 p +, 4 e -, 5 n d. 20 p +, 20 e -, 20 n e. 1 p +, 1 e -, 2 n 2. a. 13 p +, 10 e -, 15 n b. 20 p +, 18 e -, 21 n c. 28 p +, 26 e -, 31 n d. 17 p +, 18 e -, 19 n 3. a Ni b Ti c O d Cr e Br f. 7 3 Li g. h. 4. a. F b. T c. T 5. protons = 40; neutrons = 45; electrons = a (hydrogen does not) Au Foil 7. Rutherford targeted alpha particles at thin Au foil and placed a photographic detector all around the foil. α particles Nearly all the α particles went through the foil but a small number bounced back. He deduced that most of the atom is "empty" (hence most α particles pass through the foil) but there is a highly dense, positively charged, small "nucleus" (hence, a small number of α particles bounced back at sharp angles). nucleus empty space 8. <5% {since the average atomic weight of O = , then the abundance of 16 O must be close to 100% since the average weight is close to 16 and therefore the abundance of 18 O must be very close to zero otherwise the average atomic mass would be higher than 16} u; Rb {(84.912)(0.7215) + (86.909)(0.2785) = u} Ag: 51.8%, and 109 Ag: 48.2% { = (x) (1 - x); x = abundance 107 Ag; = x x; = x; x = = 107 Ag abundance; 109 Ag abundance = 1 x = = }

6 Cl = 75.5%; 37 Cl = 24.5% { = (x) (1 - x); x = abundance 35 Cl; } = x x; = x; x = = 35 Cl abundance; 37 Cl abundance = 1 x = = } Mg = 78.99%; 26 Mg = 11.01% {x = abundance 24 Mg; y = abundance 26 Mg; sum of fractional abundances: = x y; y = x; = (x) (0.1000) ( x); = x x; = x; = 1.998x; x = = 24 Mg abundance = 78.99%; 26 Mg abundance = = 11.01%} amu {AAM = (M 1 )(FA 1 ) + (M 2 )(FA 2 ) +; AAM = (46)(0.083) + (47)(0.074) + (48)(0.737) + (49)(0.054) + (50)(0.052) = 47.92amu} 14. a. {2 isotopes so 2 peaks are expected in the mass spectrum. The mass of each peak corresponds to the mass number (peaks at mass = 35 and mass = 37). The intensity of each peak reflects the relative abundance of each isotope so 35 Cl would be 75% and 37 Cl would be 25%. [The peaks need to be in a ratio of 3:1 for the 35 Cl and 37 Cl isotopes which are in a ratio of 3:1 from 75%/25% = 3:1.} b. 3 peaks { 35 Cl 35 Cl (mass = 70), 35 Cl 37 Cl (mass = 72) same mass as 37 Cl 35 Cl (mass = 72), 37 Cl 37 Cl (mass = 74)} c. Peak 70 : Peak 72 : Peak 74 = 56% : 38% : 6% ratio {peak 70 = (0.75)(0.75) = 0.56; peak 72 = (0.75)(0.25) + (0.25)(0.75) = 0.38; peak 74 = (0.25)(0.25) = 0.063} d. 75% 25% Mass 56% 38% 6% Mass a. Mn, Al b. alkaline earth metals c. fluorine, chlorine, bromine, iodine (any one of these) 16. a {NH 3 is a molecular compound (2 nonmetals) and molecular compounds have much lower melting points than ionic compounds; KBr has +1/-1 charges while BeO and MgS have +2/ charges; higher charges will yield higher melting points so drop KBr; the other ionic compounds have the same charges: Be +2 O, Mg +2 S ; to differentiate between these the smaller the ions the higher the melting point; ions higher in a column on the Periodic Table are smaller, and therefore Be +2 is smaller than Mg +2 ; likewise, O will be smaller than S ; so BeO will have the highest melting point} 17. c 18. a. nitrogen monoxide b. phosphorus trichloride c. potassium bromide d. sodium carbonate e. dinitrogen tetroxide f. potassium sulfate g. calcium phosphate h. copper(i) oxide i. manganese(ii) phosphate j. cobalt(iii) acetate k. cobalt(ii) sulfate l. potassium permanganate m. methane (common name; memorize) 19. a. SO 3 b. CaF 2 c. ClBr d. Na 2 SO 4 e. NH 4 NO 3 f. Li 2 CO 3 g. Ca(NO 3 ) 2 h. Mn 2 (SO 4 ) 3 i. CrO 3 j. TiS b

7 Polyatomic Ions, Acids, Common Names (Note: Acids and other chemicals in italics are common chemicals but may not be on the list of chemicals to be memorized!) If polyatomic ion name ends with ate then the acid (adding H + until the ion is neutral) name ends with ic acid e.g., SO 4 = sulfate H2 SO 4 = sulfuric acid If polyatomic ion name ends with ite then the acid (adding H + until the ion is neutral) name ends with ous acid e.g., NO 2 - = nitrite HNO2 = nitrous acid If ion is a single atom (e.g., Cl - ) then the ion name ends with ide (exceptions: CN -, cyanide, and OH -, hydroxide) and acid name is hydro+root+ ic acid (e.g., HCl = hydrochloric acid) NH + 4 (ammonium) H 3 O + (hydronium) OH - (hydroxide) CH 3 COO - (acetate; also written: C 2 H 3 O - 2 ) NO - 3 (nitrate) NO - 2 (nitrite) CH3 COOH (acetic acid) HNO 3 (nitric acid; strong acid) HNO 2 (nitrous acid) MnO - 4 (permanganate) CO 3 (carbonate) HCO - 3 (hydrogen carbonate) H 2 CO 3 (carbonic acid) SO 4 (sulfate) HSO - 4 (hydrogen sulfate) H 2 SO 4 (sulfuric acid; strong acid) SO 3 (sulfite) HSO - 3 (hydrogen sulfite) H 2 SO 3 (sulfurous acid) ClO - 4 (perchlorate) ClO - 3 (chlorate) ClO - 2 (chlorite) ClO - (hypochlorite) CN - (cyanide) CrO 4 (chromate) HClO 4 (perchloric acid; strong acid) HClO 3 (chloric acid) HClO 2 (chlorous acid) HClO (hypochlorous acid) HCN (hydrocyanic acid) PO 4-3 (phosphate) HPO 4 (monohydrogen phosphate) H 2 PO 4 - (dihydrogen phosphate) H 3 PO 4 (phosphoric acid) PO 3-3 (phosphite) HPO 3 (monohydrogen phosphite) H 2 PO 3 - (dihydrogen phosphite) H 3 PO 3 (phosphorous acid) F - (fluoride) Cl - (chloride) Br - (bromide) I - (iodide) NH 3 = ammonia H 2 O 2 = hydrogen peroxide CH 4 = methane C 2 H 6 = CH 3 CH 3 = ethane HF (hydrofluoric acid) HCl (hydrochloric acid; strong acid) HBr (hydrobromic acid; strong acid) HI (hydroiodic acid; strong acid) Some Common Chemicals and Common Names C 3 H 8 = CH 3 CH 2 CH 3 = propane C 4 H 10 = CH 3 CH 2 CH 2 CH 3 = butane CH 3 OH = methanol CH 3 CH 2 OH = ethanol

CHEMISTRY 103 Help Sheet #2 Atoms, Molecules, and Ions (Text: Ch 2: )

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:

More information

Chemical Nomenclature

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

More information

Naming Chemical Compounds

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:

More information

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)

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

More information

Big Idea: Matter & Atoms

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

More information

H 2 O. Chapter 9 Chemical Names and Formulas

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:

More information

Nomenclature of inorganic compounds. = naming non carbon (mostly) compounds. Some definitions:

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

More information

Experiment #4. Chemical Nomenclature

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

More information

Chapter 5: Nomenclature

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

More information

Topic 5: The Language of Chemistry

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

More information

Tustin HS AP Chemistry SUMMER ASSIGNMENT

Tustin HS AP Chemistry SUMMER ASSIGNMENT Tustin HS AP Chemistry SUMMER ASSIGNMENT Instructor: Email: Ms. Abbey Zinsser azinsser@tustin.k12.ca.us or azinsser@mytusd.org Textbook: Chemistry: The Central Science, Brown, LeMay, Bursten, 11 th edition

More information

» Composed of more than one type of atom chemically bonded.» A pure substance, meaning its properties are the same throughout the substance.

» Composed of more than one type of atom chemically bonded.» A pure substance, meaning its properties are the same throughout the substance. » Composed of more than one type of atom chemically bonded.» A pure substance, meaning its properties are the same throughout the substance.» Separated chemically not physically» No overall charge; they

More information

CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS. Chemistry 1-2 Enriched Mr. Chumbley

CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS. Chemistry 1-2 Enriched Mr. Chumbley CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS Chemistry 1-2 Enriched Mr. Chumbley SECTION 1: CHEMICAL NAMES AND FORMULAS While the bulk of the content will come from the Naming Chemical Compounds

More information

Chemical Formulas & Chemical Compounds. Chemical formula indicates the relative number of atoms of each kind in a chemical compound.

Chemical Formulas & Chemical Compounds. Chemical formula indicates the relative number of atoms of each kind in a chemical compound. Unit 6: Chemical Formulas & Chemical Compounds Chemical Names & Formulas Chemical formula indicates the relative number of atoms of each kind in a chemical compound. Molecular compound - it s formula reveals

More information

Naming Compounds. Part One: Naming Ionic Compounds. Identifying Ionic 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

More information

CHEM 103 Naming Compounds

CHEM 103 Naming Compounds CHEM 103 Naming Compounds Lecture Notes February 9, 2006 Prof. Sevian Chem 103 Please sit with your groups today. We will be doing a group problem at the end of class. 2 2005 H. Sevian 1 Agenda How we

More information

Naming Inorganic Compounds. common names systematic names

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

More information

CHEM 1105 S10 January 21, 2014

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

More information

CHEMICAL FORMULAS - NOMENCLATURE (The Language of Chemistry)

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

More information

Chapter 2. The Components of Matter

Chapter 2. The Components of Matter Chapter 2. The Components of Matter 1 The Periodic Table (Section 2.6) 13 Al 26.981 Main Idea: 1. Groups: Old numbering system: New IUPAC numbering system: 2. Periods: 3. Know the names and properties

More information

Ionic Compounds. And Acids

Ionic Compounds. And Acids CHAPTER 7 LANGUAGE OF CHEMISTRY CLASSIFICATION OF COMPOUNDS Inorganic compounds does not contain the element carbon, but there are exception to this rule, CO 2 (carbon dioxide), CO 3 2 (carbonate), and

More information

9/19/07. Chemistry 6A Fall 2007 Dr. J. A. Mack. Molar Masses. Avagagro s s Number. Avogadro s Number and the Mole

9/19/07. Chemistry 6A Fall 2007 Dr. J. A. Mack. Molar Masses. Avagagro s s Number. Avogadro s Number and the Mole Chemistry 6A Fall 007 Dr. J. A. Mack Avogadro s Number and the Mole The concept of a mole is defined so that we may equate the amount of matter (mass) to the number of particles (mole). The Standard is

More information

Chapter 9 Naming Simple Compounds

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

More information

What is the major difference between a molecular formula and formula unit?

What is the major difference between a molecular formula and formula unit? Lecture 5 Molecular Substances versus Ionic Substances Molecular Substance Ionic Substance What are some examples of molecular substances? What are some examples of ionic substances? What is the major

More information

Molecule 2 atoms chemically combined, smallest part of compound

Molecule 2 atoms chemically combined, smallest part of compound Chemical Bonds 008: Chemical Bonds Bonding: the way atoms are attracted to each other to form molecules, determines nearly all of the chemical properties we see. And, as we shall see, the number 8 is

More information

Chemical Bonding and Naming Compounds. Ionic. Acid. Base. Oct 4 7:40 PM

Chemical Bonding and Naming Compounds. Ionic. Acid. Base. Oct 4 7:40 PM Chemical Bonding and Naming Compounds (Chapter 9) Types of Bonds Ionic Bonds Molecular Bonds Types of Compounds Ionic Molecular Acid Base Chemical Bonding Atoms will bond together using their valence electrons.

More information

Chapter 5. Naming Compounds Writing Formulas

Chapter 5. Naming Compounds Writing Formulas Chapter 5 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

More information

Systematic Naming. Chapter 9. Two Types of Compounds. Two Types of Compounds 2 Ionic Compounds. Two Types of Compounds.

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

More information

Chapter 2. Chapter 2

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

More information

Nomenclature of Inorganic Compounds

Nomenclature of Inorganic Compounds Nomenclature of Inorganic Compounds Chapter 6 Hein and Arena Version 1.1 Eugene Passer Chemistry Department Bronx Community 1 College John Wiley and Sons, Inc Elements and Ions 2 The formula for most elements

More information

Naming Inorganic Compounds. common names systematic names

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

More information

Chapter 6. Naming Compounds Writing Formulas

Chapter 6. Naming Compounds Writing Formulas Chapter 6 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

More information

Chemical Nomenclature Chapter 2.5-8

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)

More information

Chapter 8 Nomenclature

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,

More information

CRHS Academic Chemistry Unit 6 - Nomenclature Practice Problems

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

More information

NOMENCLATURE AND WRITING FORMULAS

NOMENCLATURE AND WRITING FORMULAS NOMENCLATURE AND WRITING FORMULAS PART I--FORMULAS AND NOMENCLATURE OF IONIC COMPOUND Composed of Cations and Anions. Types of Cations (positive ions): A. Metals lose electrons to form positive ions. These

More information

CHEM 103 Naming Compounds

CHEM 103 Naming Compounds CHEM 103 Naming Compounds Lecture Notes February 7, 2006 Prof. Sevian 1 Agenda How we name compounds depends on what kind of compounds they are Ionic compounds Molecular compounds Acids are molecular compounds

More information

Chemical Names and Formulas

Chemical Names and Formulas Chemical Names and Formulas ELECTRONS AND THE STRUCTURE OF ATOMS BONDING AND INTERACTIONS 91 Naming Ions For students using the Foundation edition, assign problems 4, 8 15 Essential Understanding Ions

More information

Nomenclature Hint Sheet

Nomenclature Hint Sheet Nomenclature Hint Sheet The nomenclature for four different classes of compounds is covered in CH101: ionic, covalent, acid/base, and organic compounds. This document will cover ionic (chapter 4) and covalent

More information

Chapter 3 Molecules, Compounds, and Chemical Equations

Chapter 3 Molecules, Compounds, and Chemical Equations Chapter 3 Molecules, Compounds, and Chemical Equations Molecular View of Elements and Compounds 2 How do atom join together to form a compound? compounds are made of atoms held together by chemical bonds

More information

Worksheet 5 Nomenclature 1 Ionic Compounds I. Naming compounds containing only two elements (binary compounds)

Worksheet 5 Nomenclature 1 Ionic Compounds I. Naming compounds containing only two elements (binary compounds) Worksheet 5 Nomenclature 1 Ionic Compounds I. Naming compounds containing only two elements (binary compounds) 1. Name the first element. 2. Name the second element with an ide ending Example: NaCl A1

More information

Nomenclature Report. GCC CHM 151LL: Nomenclature Report GCC, 2019 page 1 of 6

Nomenclature Report. GCC CHM 151LL: Nomenclature Report GCC, 2019 page 1 of 6 Nomenclature Report Introduction Ionic Compound Nomenclature An ionic compound is described as an electrostatic attractive force between oppositely charged ions. Monoatomic Cations Metal cations are formed

More information

Inorganic Nomenclature

Inorganic Nomenclature Inorganic Nomenclature A. The Chemical Elements 1. The term INORGANIC NOMENCLATURE refers to the naming of elements and inorganic compounds. Recall that ELEMENTS are the simplest form of matter that cannot

More information

O ( ) are only used with polyatomic ions and only when there is more than one of any group. a. Examples: HNO 3. ) is incorrect; Al 2 ) 3 (SO 4

O ( ) are only used with polyatomic ions and only when there is more than one of any group. a. Examples: HNO 3. ) is incorrect; Al 2 ) 3 (SO 4 HONORS CHEMISTRY - CHAPTER 9 CHEMICAL NAMES AND FORMULAS NOMENCLATURE PACKET - V16 NAME: DATE: PAGE: I. Writing formulas of ionic compounds when given the component parts. 1. Many compounds are composed

More information

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 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

More information

Chapter 5. Molecules and Compounds. Introductory Chemistry, 3 rd Edition Nivaldo Tro 2/21/2011

Chapter 5. Molecules and Compounds. Introductory Chemistry, 3 rd Edition Nivaldo Tro 2/21/2011 Introductory Chemistry, 3 rd Edition Nivaldo Tro Chapter 5 Molecules and Compounds Based on notes of Roy Kennedy Massachusetts Bay Community College 2006, Prentice Hall Molecules and Compounds Salt Sodium

More information

Cations have a positive charge and anions have a negative charge. 3. Complete the following table.

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

More information

CHEMICAL NAMES AND FORMULAS

CHEMICAL NAMES AND FORMULAS Name Date Class 9 CHEMICAL NAMES AND FORMULAS SECTION 9.1 NAMING IONS (pages 253 258) This section explains the use of the periodic table to determine the charge of an ion. It also defines polyatomic ion

More information

Bonding and Nomenclature notes.notebook

Bonding and Nomenclature notes.notebook Chemical Bonding & Nomenclature Objectives: Distinguish between covalent and ionic bonding Explain the process of bonding Name ionic and covalent compounds and acids Write chemical formulas for ionic and

More information

Nomenclature Report. GCC CHM 151LL: Nomenclature Report GCC, 2017 page 1 of 8

Nomenclature Report. GCC CHM 151LL: Nomenclature Report GCC, 2017 page 1 of 8 Nomenclature Report Introduction Ionic Compound Nomenclature An ionic compound is described as an electrostatic attractive force between oppositely charged ions. Monoatomic Cations Metal cations are formed

More information

Ch.2: Atoms, Molecules, and Ions

Ch.2: Atoms, Molecules, and Ions Ch.2: Atoms, Molecules, and Ions Naming Recall Ionic Bond = electrostatic attraction due to the transfer of vse - s between a metal and nonmetal Covalent Bond = sharing of valence electrons between nonmetals

More information

Summary for Naming Compounds

Summary for Naming Compounds Summary for Naming Compounds 1. Group 1, 2, 3 metal with Group 15, 16, 17 nonmetals 2. Group 1, 2, 3, metal with polyatomic ions 3. Transition/other metal with Group 15, 16, 17 nonmetal 4. Transition/other

More information

OWL Assignment #2 Study Sheet

OWL Assignment #2 Study Sheet OWL Assignment #2 Study Sheet Binary Acid Nomenclature Binary compounds are composed of two elements. When one of the elements is a binary acid can be formed. Examples of this are HCl or H 2 S. When put

More information

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry Chemical Formulas and Chemical Nomenclature Mr. Matthew Totaro Legacy High School Honors Chemistry 1 Molecular View of Elements and Compounds 2 Atomic Elements Atomic Elements = elements whose smallest

More information

World of Chemistry Notes for Students [Chapter 4, page 1] Chapter 4 Nomenclature

World of Chemistry Notes for Students [Chapter 4, page 1] Chapter 4 Nomenclature World of Chemistry Notes for Students [Chapter 4, page 1] Chapter 4 Nomenclature 1) The Periodic Table Review from Chapter The elements are arranged in rows and columns on the Periodic Table according

More information

Honors Chemistry - Unit 5 Chapter 7 - Nomenclature

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

More information

CHEMISTRY 1: Chemical Bonding

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

More information

Unit 2. Atoms, Molecules, and Ions

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,

More information

The chemical formulas of most of the elements are simply their elemental symbol:

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.

More information

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry I. IUPAC Naming AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry For Ionic Compounds: Formula to Name: 1. Identify the cation (positive ion) by name, then identify the

More information

Chemical Nomenclature

Chemical Nomenclature Chemical Nomenclature Learn names you will Review: Valence electrons (the outer most electrons) are responsible for the interaction between atoms when forming chemical compounds. Another way to say that

More information

Chemistry--Unit 2: Chemical Names and Formulas Test Review

Chemistry--Unit 2: Chemical Names and Formulas Test Review vocab anion binary compound cation chemical formula formula unit ion ionic compound law of definite proportions law of multiple proportions molecular formula polyatomic ion representative particle ternary

More information

Unit 1 Physical Science: Chemical Reactions

Unit 1 Physical Science: Chemical Reactions Unit 1 Physical Science: Chemical Reactions The physical sciences are concerned with the study of inanimate natural objects. Chemistry is the study of matter, its properties, how and why substances combine

More information

Chemical Names & Formulas. Water Ammonia Methane 1

Chemical Names & Formulas. Water Ammonia Methane 1 Chemical Names & Formulas Water Ammonia Methane 1 Why Systematic Names? # atomic particles 3 (p, n, e) # elements 110+ # elements in 8 earth s crust (99%) # elements in all 25 living things # compounds

More information

Honors Chemistry - Topic IV Part I Study Guide The Language of Chemistry

Honors Chemistry - Topic IV Part I Study Guide The Language of Chemistry Honors Chemistry - Topic IV Part I Study Guide The Language of Chemistry I. Chemical Nomenclature A. Inorganic Nomenclature (pp.11132; 349-350, 554-555; 213-220) 1. Types of formulas chart showing positions

More information

4. What is the law of constant composition (also known as the law of definite proportion)?

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

More information

Naming Simple Compounds

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

More information

CHEM 1305: Introductory Chemistry

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

More information

Chemistry B11 Chapter 4 Chemical bonds

Chemistry B11 Chapter 4 Chemical bonds Chapter 4 Chemical bonds Octet rule: when undergoing chemical reaction, atoms of group 1A7A elements tend to gain, lose, or share sufficient electrons to achieve an electron configuration having eight

More information

CHAPTER 2: ATOMS, IONS, AND MOLECULES

CHAPTER 2: ATOMS, IONS, AND MOLECULES CHAPTER 2: ATOMS, IONS, AND MOLECULES Problems: 2.1-2.78, 2.81-2.93, 2.94-2.96, 2.111-2.119, 2.121, 2.127 2.1 THE NUCLEAR MODEL OF ATOMIC STRUCTURE Joseph John (J. J.) Thomson (1897) carried out experiments

More information

Compounds Element = 1 type of atom Compound = more than 1 type of atom (over 8 million) Chemical Bond = glue that links atoms together in a compound

Compounds Element = 1 type of atom Compound = more than 1 type of atom (over 8 million) Chemical Bond = glue that links atoms together in a compound Compounds Element = 1 type of atom Compound = more than 1 type of atom (over 8 million) Chemical Bond = glue that links atoms together in a compound Ionic Compounds Ionic Bonds = atoms switch e- forming

More information

Chemical Nomenclature

Chemical Nomenclature Chemical Nomenclature IUPAC International Union of Pure and Applied Chemistry. This is a group of chemists that determines, among other things, how chemicals will be named. IONIC COMPOUNDS 1. Binary Ionic

More information

1/28/13. Naming and Writing Formulas > for Ionic Compounds

1/28/13. Naming and Writing Formulas > for Ionic Compounds chemistry 1 of 29 Naming and Writing Formulas A recipe is a formula for the sauce a complete list of ingredients and their proportions. Chemistry also uses formulas. Once you know the rules, you can write

More information

Inorganic Chemical Formulation. Ms. María Isern

Inorganic Chemical Formulation. Ms. María Isern Inorganic Chemical Formulation Ms. María Isern Oxides: Combination of an element with an oxide O 2- anion To formulate: write the symbol of the element + O 2- and interchange o.n. as subscripts. To name:

More information

lost, gained or shared chemical bonds symbols subscripts NaCl, H O, CaCO, CO

lost, gained or shared chemical bonds symbols subscripts NaCl, H O, CaCO, CO Topics Chemical Bonds Force that holds atom together Stability in Bonding Valence Electrons Reactivity Types of Bonds Ionic, Metallic, Covalent, Hydrogen bond Writing Formulas and Naming Compounds Binary

More information

MgCl2 = magnesium chloride

MgCl2 = magnesium chloride Chapters 8.1 plus 7.3 and 10.4-5: Nomenclature, Writing Formulas, and Percent Composition Nomenclature Names and formulas for ionic compounds The smallest unit of an ionic compound is the formula unit

More information

2. Match a formula in the right column with its appropriate name in the left column.

2. Match a formula in the right column with its appropriate name in the left column. UNIT 3: CHEMICAL BONDING. CHEMICAL COMPOUNDS Content: Unit 3 Chemical bonding. Chemical compounds 3.1. Chemical bonding 3.2. Chemical compounds 3.2.1. Oxides 3.2.2. Hydroxides 3.2.3. Hydrides 3.2.4. Binary

More information

Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms,

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

More information

Inorganic Nomenclature

Inorganic Nomenclature Inorganic Nomenclature http://www.msu.edu/user/dynicrai/physics/h2o.htm A. The Chemical Elements 1. The term INORGANIC NOMENCLATURE refers to the naming of elements and inorganic compounds. Recall that

More information

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.

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

More information

Nomenclature (Naming Compounds) and Chemical Formulas

Nomenclature (Naming Compounds) and Chemical Formulas Nomenclature (Naming Compounds) and Chemical Formulas 1 Ions formed from a single atom Monatomic Ions Charges are determined by whether ion has lost electrons (+) or gained electrons (-) Symbols are written

More information

Unit 2. Chapter 4-Atoms and Elements, continued

Unit 2. Chapter 4-Atoms and Elements, continued CHEMISTRY 110 LECTURE Unit 2 Chapter 4-Atoms and Elements, continued I Ions II ISOTOPES-Tools A. Tools 1. Atomic number, Z,, equals the number of protons 2. Mass number, A, equals the sum of protons and

More information

629 CER Modular Laboratory Program in Chemistry

629 CER Modular Laboratory Program in Chemistry M I S C 629 CER Modular Laboratory Program in Chemistry editor: M. L. Gillette Naming Inorganic Chemical Substances prepared by M. L. Gillette, Indiana University Kokomo, and H. A. Neidig, Lebanon Valley

More information

Chapter 6 Inorganic and Organic Compounds: Names and Formulas

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

More information

Nomenclature. Ex. For sodium the oxidation number is +1. For oxygen the oxidation number is -2.

Nomenclature. Ex. For sodium the oxidation number is +1. For oxygen the oxidation number is -2. Nomenclature 1. BONDING CAPACITY (VALENCE) The number of bonds an atom can make. For a Cation, the bonding capacity is the number of electrons lost to become stable. For an Anion, the bonding capacity

More information

Naming and Counting Atoms and Molecules. Chemistry--Unit 2

Naming and Counting Atoms and Molecules. Chemistry--Unit 2 Naming and Counting Atoms and Molecules Chemistry--Unit 2 Masses of 22.4 L O 2, N 2, & HCl N 2 28 g O 2 32 g HCl 36.5 g Observation: At 1 atmosphere pressure and 0 o C, 22.4 L of 3 different gases have

More information

Chemical Formulas Types of chemical formulas [X m Y n ]

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

More information

Books at Amazon.com on Nanotechnology

Books at Amazon.com on Nanotechnology Books at Amazon.com on Nanotechnology http://www.amazon.com/s/103-9040246- 0256655?ie=UTF8&keywords=NANOTECHNOLOGY%20&tag =thenanotecinscie&index=books&search=search&link%5fcode=qs Ions Ions are charged

More information

Ionic Compound Formulas.

Ionic Compound Formulas. Ionic Compound Formulas www.lab-initio.com Valence Electrons Electrons are divided between core and valence electrons B 1s 2 2s 2 2p 1 Core = [He], valence = 2s 2 2p 1 Br [Ar] 3d 10 4s 2 4p 5 Core = [Ar]

More information

Ions and Ionic Compounds

Ions and Ionic Compounds Ions and Ionic Compounds Elements combine in a specific ratio to form compounds. Compounds can be categorized as ionic or covalent depending on the type of bond present within the compound. Ionic compounds

More information

Nomenclature. Why, Learn it? History:

Nomenclature. Why, Learn it? History: Nomenclature Why, Learn it? Allow us to be able to name compound we have never seen before. If we know the name of a compound we can determine its formula. We can look at a formula, determine it name and

More information

Chapter 5 Molecules and Compounds

Chapter 5 Molecules and Compounds Chapter 5 Molecules and Compounds 1 Chemical Formulas Atomic/Molecular Elements Ionic/Molecular Compounds Naming Ionic Compounds Naming Molecular Compounds Naming Acids Formula Mass Atomic / Molecular

More information

Nomenclature. Symbols for Atoms, Molecules, and Ions. Ion Example: Ionic Bonding: Atoms:

Nomenclature. Symbols for Atoms, Molecules, and Ions. Ion Example: Ionic Bonding: Atoms: Symbols for Atoms, Molecules, and Ions Nomenclature (Naming) Chemistry 11 Atoms: Remember: the atomic number = # of protons The atomic number = # of electrons in a neutral element # of neutrons = mass

More information

Why does an element want to bond?

Why does an element want to bond? Why does an element want to bond? State 3 differences between ionic vs. covalent compounds What is a chemical formula? It indicates the relative number of atoms of each kind in an ionic compound. Ex Al

More information

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

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"

More information

Chapter 2: Atoms, Molecules, and Ions

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

More information

CHAPTER 7: LANGUAGE OF CHEMISTRY

CHAPTER 7: LANGUAGE OF CHEMISTRY CHAPTER 7: LANGUAGE OF CHEMISTRY Problems: 3-12, 13(a-c), 14(a,c,d), 15(a-c), 16(a,c), 17-19, 20c, 21, 22(a,c), 23-27, 33(a,c,d), 34(a,c,d), 35, 36(a,c), 37(a,b,d), 43-48, 49b, 50b, 51-52, 59-62 7.1 CLASSIFICATION

More information

Name: Lab Section: Prepared by. Dr. Gary Evett, Professor of Biophysical Sciences, WNC-Fallon Campus. Edited by

Name: Lab Section: Prepared by. Dr. Gary Evett, Professor of Biophysical Sciences, WNC-Fallon Campus. Edited by Chemical Nomenclature Name: Lab Section: Date: Sign-Off Prepared by Dr. Gary Evett, Professor of Biophysical Sciences, WNC-Fallon Campus Edited by Dr. Steve Carman, Professor of Biophysical Sciences, WNC-Carson

More information

Chapter 6 and 15 Ionic Compounds

Chapter 6 and 15 Ionic Compounds Chapter 6 and 15 Ionic Compounds Chapter 6 Ionic compounds 6.3, 6.4 6.1: Intro to Chemical Bonding A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different

More information

Unit II: Atoms Molecules & Ions

Unit II: Atoms Molecules & Ions Unit II: Atoms Molecules & Ions A. B. C. D. The Periodic Table Why and how compounds form Rules for writing ions Writing formulas and naming compounds 1. 2. 3. Binary compounds Non-binary compounds Formula

More information