CHEM1405 LAB4

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Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez I. Objectives • To learn about chemical symbols of atoms and isotopes • To practice naming ionic and molecular compounds II. Introduction Part 1: Atoms ______________________________________________________________________ Atoms are the submicroscopic particles that constitute the fundamental building blocks of ordinary matter. The atomic model states that atoms have three subatomic particles which are electrons, neutrons, and protons. The Atomic Number (Z) is the number of protons in the nucleus of the atom and also defines the element. For example, any atom with 6 protons is Carbon, and any atom with 8 protons is oxygen. Since atoms are electrically neutral the atomic number also equals the number of electrons unless otherwise stated. The Mass number (A) is the total number of protons and neutrons in an atom. Figure 1 displays how the chemicals are symbolized and how they incorporate mass number and atomic number. Figure 1. Chemical symbols Part 2: Chemical Nomenclature_________________________________________________________ Free atoms are rare in nature; instead they bind together in specific geometrical arrangements to form molecules. All the atoms in a molecule move as one unit. The naming of compounds is called chemical nomenclature. It is a very specific process, depending on the type of compound. The rest of this introduction section describes how to name ionic compounds, molecular compounds, hydrates, and acids. Nomenclature of Ionic Compounds Ionic compounds are composed of ions. An ion is an atom or molecule with an electrical charge. Monatomic ions are formed from single atoms that have gained or lost electrons. Polyatomic ions are formed from molecules (groups of atoms bonded together) that have gained or lost electrons. Atomic number (Z) = number of protons = number of electrons (if neutral) (4.1) mass number (A) = number of protons + number of neutrons (4.2) A – Z = number of neutrons (4.3) All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Negative ions are called anions, and are formed when an atom or molecule gains electrons. All non- metals form negatively charged ions. Positive ions are called cations, and are formed when an atom or molecule loses electrons. All metals form positively charged cations. Ions with opposite charges (positive metal cations and negative non-metal anions) will experience a strong electrostatic attraction and form an ionic bond, which leads to the formation of the ionic compound. Non-metal Anions Non-metals will form anions with only one possible negative charge. The following Periodic Table shows the charges for non-metal anions commonly found in ionic compounds: Note that • The magnitude of the negative charges on these anions is equal to 8 minus their Group Number. • The names of these anions are based on the element names, but the endings are all changed to –ide. Metal Cations Most (but not all) main group metals will form cations with only one possible charge. Most (but not all) transition metals will form cations with more than one possible charge. The following Periodic Table shows the charges for metal cations commonly found in ionic compounds: Example 4.1 Sulfur in Group 6A forms anions with a [8–6]=2, or, –2 charge. Example 4.2 The Cl -1 anion is called the chloride ion. All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Note that • The magnitude of the positive charge on the main group metal cations is generally equal to their Group Number. • The names of metal cations with only one possible charge are the same as the names of the metals themselves. • For metal cations with more than one possible charge, the ion charge must be indicated in the ion name. In the IUPAC system, the ion charge is indicated in the name as Roman numerals in brackets. Polyatomic Ions Polyatomic ions are formed from molecules (groups of atoms bonded together) that have gained or lost electrons. The table below includes a list of common polyatomic ions. Example 4.3 Magnesium in Group 2A forms cations with a +2 charge. Example 4.4 Al +3 is called the aluminum cation. Ag +1 is called the silver cation. Example 4.5 Pb +2 is called the lead(II) cation. Pb +4 is called the lead(IV) cation. OH − 1 Hydroxide O 2 − 2 Peroxide CN − 1 Cyanide CO 3 − 2 Carbonate SCN − 1 Thiocyanate SO 3 − 2 Sulfite HCO 3 − 1 Bicarbonate (Hydrogen Carbonate) SO 4 − 2 Sulfate All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

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Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Note that • Almost all the polyatomic ions are negatively charged anions. • Most of the names of polyatomic anions end in either –ate or –ite. The –ate’s always have one more oxygen than the -ite’s. Formulas and Names of Ionic Compounds Ionic compounds are formed when positive cations and negative anions are attracted to each other via strong electrostatic forces. This attraction is called an ionic bond. The following are the basic rules for writing the formulas and names of ionic compounds: Writing Formulas 1. Determine the formulas and charges on the cation and anion involved in the compound. 2. Combine the ions in a ratio that results in the formation of a neutral ionic compound. In other words, the total charge of all the positive cations must equal the total charge of all the negative anions in the compound. The numbers of each element present in the compound are shown as subscripts after the element symbol. Writing Names 1. Both the cation and anion must be named. 2. Always name the cation first, then the anion. HSO 3 − 1 Bisulfite (Hydrogen Sulfite) S 2 O 3 − 2 Thiosulfate HSO 4 − 1 Bisulfate (Hydrogen Sulfate) C 2 O 4 − 2 Oxalate C 2 H 3 O 2 − 1 Acetate CrO 4 − 2 Chromate NO 2 − 1 Nitrite Cr 2 O 7 − 2 Dichromate NO 3 − 1 Nitrate MnO 4 − 1 Permanganate PO 3 − 3 Phosphite ClO − 1 Hypochlorite PO 4 − 3 Phosphate ClO 2 − 1 Chlorite ClO 3 − 1 Chlorate NH 4 +1 Ammonium ClO 4 − 1 Perchlorate Hg 2 +2 Mercury (I) Example 4.6 Sulfate, SO 4 − 2 , has one more oxygen atom present than sulfite, SO 3 − 2 . All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Note in the above Example 9 that parentheses are placed around the polyatomic portion of compound, to indicate that it must be treated as a complete and whole unit. Example 4.7: Write the formula and name for the compound formed between calcium and fluorine Ca (metal) forms a +2 cation Ca +2 , the calcium cation. F (non-metal) forms a -1 anion F − 1 , the fluoride anion. To obtain a neutral compound, 1 Ca +2 is needed for every 2 F − 1 The formula of the compound is CaF 2 The name of the compound is Calcium Fluoride Example 4.8: Write the formula for iron(III) chloride. First identify the cation and the anion in this compound. Cation = iron(III) = Fe +3 (transition metal cation) Anion = chloride = Cl − 1 (non-metal anion) To obtain a neutral compound, 1 Fe +3 is needed for every 3 Cl − 1 The formula of the compound is FeCl 3 Example 4.9: Write the formula for magnesium phosphate. First identify the cation and anion in this compound. Cation = magnesium = Mg +2 (metal cation) Anion = phosphate = PO 4 − 3 (polyatomic anion) To obtain a neutral compound, 3 Mg +2 are needed for every 2 PO 4 − 3 The formula of the compound is Mg 3 (PO 4 ) 2 Example 4.10: Name the ionic compound Al(NO 3 ) 3 First identify the cation and anion in this compound. Cation = Al +3 = the aluminum cation (metal cation) Anion = NO 3 − 1 = the nitrate anion (polyatomic anion) The name of this compound is Aluminum Nitrate All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Nomenclature of Simple Covalent Compounds Covalent compounds are compounds formed between non-metals only. Simple binary covalent compounds contain just two different types of non-metal elements. When non-metals combine they can form several different covalent compounds. These compounds must therefore be identified with unique names and formulas. Formulas and Names of Simple Covalent Compounds 1. Always write/name the element with more metallic character first. Metallic character increases going from right to left, and top to bottom on the Periodic Table. 2. Then write/name the second (less metallic) element, changing the ending of its name to -ide. 3. Since nonmetals often combine in different proportions to form a number of different compounds, prefixes must be included in the names to indicate the numbers of each kind of atom present.Prefixes for 1-10 atoms are given in the following table. Example 4.11: Name the compound TiO 2 First identify the cation and anion in this compound. Cation = Ti +4 = the titanium(IV) cation (transition metal cation) Anion = O − 2 = the oxide anion (non-metal anion) The name of the compound is Titanium(IV) Oxide Example 4.12: Carbon and oxygen combine to form two common covalent compounds CO 2 and CO. Number Prefix Number Prefix 1 Mono 6 Hexa 2 Di 7 Hepta 3 Tri 8 Octa 4 Tetra 9 Nona 5 Penta 10 Deca Example 4.13: A compound contains 3 atoms of sulfur and 4 atoms of phosphorus. Write its name and formula. Since phosphorus is the more metallic element (left of sulfur), it must be named first. Sulfur being the less metallic element is named second with an -ide ending = sulfide . The prefix for three is tri , and the prefix for four is tetra . The name of this compound is tetraphosphorus trisulfide The formula of this compound is P 4 S 3 All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

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Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez There are two important exceptions to the naming rules outlined so far: • Never use the prefix “mono” for the first element, even if just one atom is present. • Never use any prefixes at all for simple covalent compounds containing Hydrogen. Please note that many simple covalent compounds have common, rather than systematic names. Please memorize the common names of the following three compounds: • H 2 O water • NH 3 ammonia • CH 4 methane Covalent compounds containing more than two non-metal elements become increasingly more difficult to name, and common names for these compounds are more extensively used. You will not have to learn these yet. Nomenclature of Acids Acids are compounds that release hydrogen cations ( H +1 ) when dissolved in water. They are all found in the aqueous state (aq). Example 4.14: Write the name of the compound N 2 O . The two N atoms require the prefix di in the name. The one O atom requires the prefix mono in the name. The ending of oxygen must be changed to –ide = oxide . The name of this compound is dinitrogen monoxide Example 4.15: Write the name of the compound BCl 3 Although just one B atom is present, the prefix mono is not used since it is the first element in this compound. The three Cl atoms require the prefix tri in the name. The ending of chlorine must be changed to –ide = chloride . The name of this compound is boron trichloride Example 4.16: HF is hydrogen fluoride not hydrogen monofluoride or monohydrogen monofluoride. HCl (aq)  H +1 (aq) + Cl -1 (aq) hydrochloric acid  hydrogen ions + chloride ions (4.4) (4.5) HNO 3 (aq)  H +1 (aq) + NO 3 -1 (aq) nitric acid  hydrogen ions + nitrate ions (4.6) (4.7) All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez In acids the element hydrogen actually behaves like a Group 1A metal cation. Since it behaves like a +1 cation, hydrogen is always written first in the formulas of all acids. The anion in the acid can be either monatomic or polyatomic, and affects how the acid is named. Acids containing Non-Metal Anions These acids contain the H +1 cation and a monatomic non-metal anion. Acids containing monatomic anions are named using the prefix hydro + the name of the anion with the suffix -ic + the word acid. The formulas of these acids are obtained in an identical fashion to regular ionic compounds. The H +1 cation and the monatomic anion are combined in a ratio to yield a neutral compound. Acids containing Polyatomic Anions These acids contain the H +1 cation and a polyatomic anion. These acids have names that are based on the name of the polyatomic ion in the acid. If the polyatomic ion has the ending -ate, in the acid the ending is changed to -ic + acid. If the polyatomic ion has the ending -ite, in the acid the ending is changed to -ous + acid. H 2 SO 3 (aq)  2 H +1 (aq) + SO 3 -2 (aq) sulfurous acid  hydrogen ions + sulfite ions (4.8) (4.9) Example 4.17: Hydrochloric acid, HCl (aq), contains H +1 and the monatomic anion, chloride, Cl − 1 . Example 4.18: Name the acid HBr (aq). This acid contains H +1 and the monatomic anion, bromide , Br − 1 . The name of this acid is hydro + brom- ic + acid = hydrobromic acid Example 4.19: Write the formula and name for the acid containing the phosphide anion. This acid contains H +1 and the P − 3 anion (monatomic). Just combine them together like any other cation and anion: 3 H +1 : 1 P − 3 The formula of this acid is H 3 P (aq) H 3 P (aq) is named hydro + phosphor- ic + acid = hydrophosphoric acid Example 4.20: Nitric acid, HNO 3 (aq), contains H +1 and the monatomic anion, nitrate, NO 3 − 1 . All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Again, the formulas of these acids are obtained in an identical fashion to regular ionic compounds. The H +1 cation and the polyatomic anion are combined in a ratio to yield a neutral compound. Nomenclature of Hydrates A hydrate is typically an ionic compound with a certain number of water molecules loosely bound to it. The general formula of a hydrate is MX ⋅ nH 2 O (s), where M is the cation in the ionic compound, X is the anion in the ionic compound and nH 2 O are the water molecules loosely bound to the ionic compound. Hydrates are named by writing the name of the ionic compound first, followed by the word “hydrate”. To indicate the number of water molecules present, prefixes must be used. Example 4.21: Name the acid HClO 3 (aq). This acid contains H +1 and the polyatomic anion ClO 3 − 1 = chlorate . To name this acid, the ending - ate is switched to - ic . The acid HClO 3 (aq) is thus called chloric acid Example 4.22: Name the acid H 2 SO 3 (aq). This acid contains H +1 and the polyatomic anion SO 3 − 2 = sulfite . To name this acid, the ending -ite is switched to -ous . The acid H 2 SO 3 (aq) is thus named sulfurous acid Example 4.23: Write the formula for oxalic acid. Oxalic acid must contain (by reverse logic) the polyatomic anion oxalate = C 2 O 4 − 2 , as well as H +1 (the cation in all acids). Once the ions have been identified, just combine them together like any other cation and anion: 2 H +1 : 1 C 2 O 4 − 2 The formula of oxalic acid is H 2 C 2 O 4 (aq) Example 4.24: Name the hydrate MgSO 4 ⋅ 7H 2 O . MgSO 4 is the ionic compound magnesium sulfate . Since there are seven water molecules present, the correct prefix to use is hepta . The name of this hydrate is magnesium sulfate heptahydrate All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

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Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez The water molecules in a hydrate can be removed with relative ease by heating the hydrate. The ionic compound that remains after heating is called an anhydrous salt. Often the anhydrous salt has a completely different color and texture from the hydrate. Example 4.25: Write the formula for copper(II) chloride dihydrate. Copper(II) chloride has the formula CuCl 2 The prefix di indicates that there are two water molecules present. The formula of this hydrate is CuCl 2 ⋅ 2H 2 O MX ⋅ nH 2 O (s)  MX (s) + nH 2 O Hydrate ⟶ Anhydrous salt + Free Water (4.10) (4.11) Example 4.26: Copper(II) sulfate pentahydrate is blue and crystalline, whereas anhydrous copper(II) sulfate is white and powdery All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez III. Procedure Part 1: Atoms ___________ ___________________________________________________________ 1. The periodic table has a great deal of information about every atom. Using your periodic table, complete Table 1. 2. To test your knowledge of isotopes, draw arrows between all pairs of atoms in the table above that are isotopes of each other. Part 2: Chemical Nomenclature_________________________________________________________ 3. Write formulas/charges or names as appropriate for each of the monatomic ions and ionic compounds in Table 2. 4. Write formulas or names as appropriate for each of the covalent compounds and acids in Table 3. 5. Write formulas or names as appropriate for each of the hydrates in Table 4. All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez IV. Data Collection Part 1: Atoms ___________ ___________________________________________________________ Table 1. Atomic structure of atoms and isotopes Name Symbol Atomic number Mass Number Number of neutrons Number of Electrons Charge hydrogen-1 1H + 1 1 0 1 +1 Dihydrogen 2H 1 1 0 1 0 sodium-22 22Na + 11 22 11 10 +11 Magnesium Mg 12 24 12 12 0 Magnesium-25 25Mg 12 25 13 13 -1 Titanium-47 47Ti -4 22 47 25 26 -4 Silver-108 108Ag + 47 108 61 46 +1 Flourine-19 19F 9 19 10 9 0 carbon-13 13C 6 13 7 6 0 carbon-12 C 6 12 6 6 0 carbon-13 13C 6 13 7 7 -1 carbon-14 14C 6 14 8 5 +1 Helium 4He + 2 4 2 1 +1 Oxygen O-2 8 16 8 10 -2 argon-41 41Ar 18 41 23 18 0 Galium-70 70Ga 31 70 39 31 0 All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

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Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Part 2: Chemical Nomenclature_________________________________________________________ Table 2. Ions and Ionic Compounds Galium-70 70Ga +3 31 70 39 28 +3 Boron B 5 10 5 2 +3 Boron-11 11B 5 11 6 5 0 Formula/Charge or Name Calcium ion Ca+2 Phosphide ion P-3 Iodide ion I- Gallium ion Ga+3 Titanium(IV) ion Ti+4 C − 4 Carbon Ion Rb +1 Rubidium Ion Pb +4 Lead Ion S − 2 Sulfer Ion Cr +2 Chromium Ion Magnesium nitride Mg2N2 Lithium oxide Li2O Aluminum sulfite Al2S3 All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Table 3. Covalent Compounds and Acids Copper(II) bicarbonate CuCO3 Sodium nitrate NaNO3 SrI 2 Strontium Iodide Ba 3 (PO 4 ) 2 Barium Phosphate (NH 4 ) 2 O Ammonium Oxide Fe(ClO) 3 Iron(III) Hypocholorite ZnCrO 4 Zinc Chromate Formula or Name Dichlorine monoxide Cl2O Disulfur dichloride S2Cl2 Carbon tetrafluoride CF4 Phosphorus pentachloride PCl4 Nitrogen tribromide NBr3 AsI 3 Arsenic Triiodide P 4 O 10 Tetraphosophorus Decoxide All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Table 4. Hydrate compounds Cl 2 O 7 Dichlorine Heptoxide SeCl 6 Selenium Hexachloride NO Nitrogen Oxide Hydroiodic acid HI Carbonic acid H2CO3 Chlorous acid HClO2 Sulfuric acid H2SO4 Phosphorous acid H3PO3 HCN (aq) Hydrocyanic Acid H 2 C 2 O 4 (aq) Oxalic Acid HNO 2 (aq) Nitrous Acid H 2 Cr 2 O 7 (aq) DiChromic Acid HMnO 4 (aq) Permanganic Acid Formula or Name Magnesium sulfate heptahydrate MgSO4 . 7H2O Copper(I) sulfate pentahydrate CuSO4 . 5H2O Potassium phosphate decahydrate K3PO4 . 10H2O Calcium chloride hexahydrate CaCl2 . 6H2O Iron(III) nitrate nonahydrate Fe(NO3)3 . 9H2O CoSO 4 ⋅ H 2 O Cobalt(II) Sulfate Monohydrate Na 2 CrO 4 ⋅ 4H 2 O Sodium Chromate Tetrahydrate CuF 2 ⋅ 2H 2 O Copper(II) Flouride Dihydrate Sr(NO 3 ) 2 ⋅ 6H 2 O Sodium Nitrate Hexahydrate ZnSO 4 ⋅ 7H 2 O Zinc Sulfate Heptahydrate All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

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Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez V. Applied Exercises Complete the following table. Classify the type of compound and write the name or formula as appropriate. Classification Name or Formula C 3 O 2 Covalent compound Tricarbon Dioxide IF 7 Covalent compound Iodine Heptaflouride Rb 2 CO 3 Covalent Compound Rubidium Carbonate SnS 2 Ionic Compound Tin(IV) Sulfide Au(CN) 3 Ionic Compound Gold(III) Tricyanide H 2 CrO 4 (aq) Aqueous Acid Chromic Acid H 3 P (aq) Aqueous Acid Phosphoric Acid Li 3 PO 4 Ionic Compound Lithium Phosphate Mg 3 N 2 Ionic Compound Magnesium Nitride Ti(C 2 H 3 O 2 ) 4 Ionic Compound Titanium(IV) Asetate Fe 2 O 3 Ionic Compound Ferric Oxide NaH Ionic Compound Sodium Hydride Br 3 O 8 Covalent compound Tribromine Octoxide MnS 2 O 3 Ionic Compound Manganese(II) Thiosulfate NH 4 NO 2 Ionic Compound Ammonium Nitrite Cd(ClO 2 ) 2 Ionic Compound Cobalt(II) Chlorate Ba(HSO 3 ) 2 Ionic Compound Barium Hydrogen Carbonate Cu 2 O Ionic Compound Copper(I) Oxide NiBr 3 Ionic Compound Nickel(III) Bromide Sr(OH) 2 Ionic Compound Strontium Hydoxide Perchloric acid Aqueous Acid HClo4 Potassium permanganate Ionic Compound KMnO4 Calcium hydride Ionic Compound CaH2 Vanadium(II) bicarbonate Ionic Compound V2(CO3)3 All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Answer the following questions using COMPLETE sentences. 1. How are the following types of compounds recognized from their formulas? • Ionic: An ionic bond is between a metal and a non-metal. • Covalent: In a covalent bond is between two or more non-metals. • Acid An Acid has a hydrogen atom in front of the molecular formula. 2. When do parentheses appear in the formulas of ionic compounds? Parenthesis appear in the formulas of ionic compounds when it contains more than one polyatomic molecule. 3. Do Roman Numerals appear in the names of ionic or covalent compounds? Explain why they are used. Bismuth(V) nitrate Ionic Compound Bi(NO3)3 Rubidium peroxide Ionic Compound Rb3O2 Strontium hydrogen phosphite Ionic compound Sr(HPO3)2 Hydrofluoric acid Aqueous Acid HF Chromium(III) thiocyanate Ionic compound C3CrN3S3 Acetic acid Aqueous Acid CH3COOH Molybdenum(IV) carbonate Ionic compound Mo(CO3)2 Tetraiodine nonaoxide Covalent Compound I4O9 Diphosphorus tetrafluoride Covalent Compound P2F4 Aluminum sulfate Ionic compound Al2(SO4)3 Ammonium hydroxide Ionic compound NH4OH Sodium dichromate Ionic compound Na2Cr2O7 Carbon disulfide Covalent Compound CS2 Nickel(II) oxalate Ionic compound NiC2O4 Barium selenide Ionic compound BaSe Silver bisulfate Ionic compound AgHO4S All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

Lab 4: Chemical Symbols and NomenclatureIntroductory Chemistry – Prof. Martinez Roman Numerals appear in the names of covalent compounds. This is because some metals have multiple isotopes and therefore different charges. 4. Do Greek Prefixes appear in the names of ionic or covalent compounds? Explain why they are used. Greek prefixes appear in the names of covalent compounds. The prefixes are used to determine how many atoms of each element are in the formula. 5. What is the relationship between the number of hydrogens in an acid and the charge on the anion that they are combined with? Hydrogen is equal to one positive charge, so for every Hydrogen, the corresponding anion has one negative charge. All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For more information, please contact me at Esmeralda.Martinez@lonestar.edu

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