Atoms, Elements, The Periodic Table & Nomenclature

Atoms, Elements, The Periodic Table & Nomenclature

Democritus & Atomism Developed a theory called “Atomism.” This theory was originally envisioned by his teacher Leucippus to account for the materialistic nature of the world. “The laughing philosopher” c. 460 BCE (Abdera) The Father of Atomism The atomists held that everything tangible is composed of small indivisible bodies which they called “atoms” and that these atoms move

Antoine Lavoisier Defined a chemical “element” as a substance that cannot be decomposed into simpler substances by chemical means. Created a table of 33 of the then known elements. 1743 (Paris) – 1794 (Paris) “The Father of Modern Chemistry” Grouped the elements into four categories based on their physical and chemical

Jöns Jakob Berzelius Developed a table of atomic weights in 1828. Introduced the use of letters as symbols for the elements. Determined the atomic weight of 43 elements. First to isolate pure calcium, barium, strontium, silicon, titanium, and zirconium. Swedish chemist 1779 – 1848 Discovered selenium, thorium, and cesium.

Johann Döbereiner In 1817, he proposed “triads,” or groups of three elements with similar properties. He later published these ideas in 1829. Examples of triads: lithium, sodium, & potassium; calcium, strontium, & barium; chlorine, bromine, & iodine. Discovered that the relative atomic mass of German Scientist 1780–1849

John Newlands Proposed the “Law of Octaves.” 1837 (London) – 1898 H1 Li 2 Be 3 B4 C5 N6 O7 F8 Na 9 Mg 10 Al 11 Si 12 P 13 S 14 Cl 15 K 16 Ca 17 Cr 19 Ti 18 Mn 20 Fe 21 In 1863, he arranged the 62 known elements in order of their atomic weights and observed similarities between the first and ninth and second and tenth elements, etc. Newlands’ Periodic Table Co & Ni 22 Cu 23 Zn 24 Y 25 In 26 As 27 Se 28 Br 29 Rb 30 Sr 31 Ce & La 33 Zr 32 Bi & Mo 34 Rh & Ru 35 Pd 36 Ag 37 Cd 38 U 40 Sn 39 Sb 41 Te 43 I 42 Cs 44 Ba & V 45 Ta 46 W 47 Nb 48 Au 49 Pt & Ir 50 Os 51 Hg 52 Tl 53 Pb 54 Bi 55 Th 56

Lothar Meyer German chemist 1830 – 1895 In 1869, he compiled a periodic table of 56 elements based on the “periodicity” of their properties (e.g., molar volumes) when arranged in order of increasing

Meyer’s Periodic Table for Molar Volume

Dmitri Mendeleev “Father of the Modern Periodic In 1869,Table” he produced a table based on the atomic weights. He actually arranged them such that elements with similar properties were located in the table Russian Physicist and Chemist underneath each other; thus, making it easier 1834 (Tobolsk, Siberia ) – 1907 (St. Petersburg) to observe the “periodicity.”

Mendeleev’s Periodic Table

1 2 3 4 5 6 Periods are shown as horizontal rows. All of the elements in a given period have the same number of atomic shells.

Groups or families are shown as vertical columns. There are 18 groups in the periodic 1 7 8 table. 2 3 4 5 6 Elements in a group have similar electronic configurations for their valence shell electrons. This is why elements in a group have similar chemical properties.

William Ramsay Discovered argon in 1894. Discovered the noble gases which formed a new group in the periodic table. Awarded the Nobel Prize for Chemistry in 1904. 1852 (Glasgow) – 1916 (High Wycombe)

Henry Moseley In 1914, he determined the atomic number of each of the elements by x-ray scattering. English physicist 1887 – 1915 He modified the “periodic law” to indicate that the properties of the elements vary periodically with their atomic number rather than atomic weight.

Henry Moseley He pointed out the existence of missing elements in the periodic table for atomic numbers 43, 61, 72, and 75. Each of these elements, Tc, Pm, Hf, and Re were eventually He also showed that there are no elements discovered. lighter than hydrogen (Z 1) and that there is no possibility for elements between hydrogen and helium (Z 2). Both possibilities had been advanced, with some proposals demanding three elements between

Glenn Seaborg Starting in 1940, he synthesized several of the transuranic elements that occur after uranium in the periodic table. American chemist 1912 – 1999 He won the Nobel Prize for Chemistry in 1951 for the discovery of plutonium. Seaborgium (element

th r a E ne tals M i l i a e al k l k M A Al ls a et Periodic Table Transition metals Lanthanide Series Actinide Series ns e g lo bl a H No e as eG s

Nomenclature Rules Rules for naming three classes of compounds: ionic compounds, binary covalent What type of compound is it? compounds & acids. IONIC COMPOUND: Composed of cations (metals or polyatomic ions) and anions (nonmetals or polyatomic ions). TYPE I: Only one type of cation is observed. COVALENT COMPOUND: Nonionic – not composed of cations & anions. Generally, only nonmetals are present. TYPE II: More than one type of cation is observed. TYPE III: Covalent, nonionic. ACID: Produces H in water. Typically the hydrogen cation is written first in the chemical formula. ACIDS: Anion does not contain oxygen. OXYACIDS: Anion does contain oxygen.

Rules for Naming Ionic Compounds Determine whether or not the compound 1.) is ionic. How do you know the compound is ionic in the first place? a.) If the compound contains a metal, then it is most likely an ionic compound. Metals readily lose electrons to form positive ions, called cations. Ionic compounds almost always contain a metal as andnot a nonmetal an anion.will b.)a cation However, all ionicascompounds contain a metal cation. The cation could be a polyatomic ions, such as NH4 .

Rules for Naming Ionic Compounds Determine whether there is only one type 2.) of cation possible (Type I) or whether there are several a.) If the cation is a polyatomic ion cations possible (Type II). (e.g., ammonium, NH4 ), then there is only one possible charge and so it is a type I compound. b.)Alkali If themetals cation(Group is a metal, determine 1A) 1 if it cation forms only one type of cation. Alkaline earth metals (Group 2A) 2 cation Transition metals (Group 1-8B) often form more than one type of

Rules for Naming Type I The cation Compounds is named first and the anion 1.) is named second. 2.) The name of the cation is the same as the name of the element. So both the element Mg and the cation Mg2 are called magnesium. (Note: For polyatomic cations, you must memorize the names. ) 3.) The anion is named by taking the root name of the element and adding the suffix ide. For example, F is an atom of fluorine and F- is the anion fluoride. (Note: For polyatomic anions, you must memorize the names. )

Rules for Naming Type I Compounds with polyatomic ions Polyatomic ions then resemble molecules in that they contain at least two atoms bound together in a definite arrangement. The steps for naming compounds with polyatomic ions: 1.) The cation is listed first and the anion second. 2.) The polyatomic ion names must be memorized. 3.) No extra prefixes or suffixes are

Table of Polyatomic Ions Symbol (root) per-root-ate root-ate root-ite hypo-root-ite Cl (chlor) ClO4 BrO4 IO4 - ClO3 BrO3 IO3 NO3 CO3 2SO4 2SeO4 2PO4 3AsO4 3- ClO2 BrO2 IO2 NO2 - ClO BrO IO XXX XXX SO3 2SeO3 2PO3 3AsO3 3- XXX CrO4 2- XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX XXX - 1 2 3 4 5 6 7 8 9 10 Cr (Chrom) 11 12 Mn (mangan) Ti (titan) 13 14 15 16 Acetate** Formate** Oxalate** Cyanate XXX 17 18 Thiocyanate*** Thiosulfate*** XXX Br (brom) I (iod) N (nitr) C (carbon) S (sulf) Se (selen) P (phosph) As (Arsen) XXX XXX * XXX XXX XXX dichromate 2- Cr2O7 MnO4XXX XXX XXX XXX XXX - TiO3 2- C2H3O2 CHO2 C2O4 2NCO SCN S2O3 2- - XXX XXX XXX XXX * Sulfur has two anions that are often referred to as persulfate. They are peroxomonosulfate (or peroxymonosulfate) ion, SO5 2- and peroxodisulfate (or peroxydisulfate) ion, S2O8 2-. **The organic anions. *** Thiocyanate and thiosulfate are formed by substituting a sulfur for an oxygen into the cyanate and sulfate ions.

Nomenclature Mnemonic for Remembering “ates” Nick the Camel Ate a Clam Supper and Crepes (for dessert) in Phoeni

Nomenclature Mnemonic for Remembering “ates” Nick the Camel Ate a Clam Supper and Crepes (for dessert) in Phoeni Consonants Vowels Polyatomic Nick Nitrate Oxygen 3 – Ion NO 3 Camel Carbonate CO3 2Clam Chlorate ClO3 (Note: Charge-1 3 -2 3 -1 Bromate and Iodate are the same as Chlorate.) Supper Sulfate SO4 2Crepes chromate CrO4 2- 4 -2 4 -2

Rules for Naming Type II Additionally forCompounds Type II Compounds: 4.) Use a roman numeral after the cation to indicate the ionic charge of that cation. So FeO would be called iron(II) oxide since the cation is Fe2 and Fe2O3 would be iron(III) oxide since the cation is Fe3 . 5.) Alternatively, when using traditional names atoms whose valence numbers vary, you add the suffix –ous to the one with the lower valence state and –ic to the one with the higher valence state. So FeO would be called ferrous oxide since the cation is Fe2 and Fe2O3 would be ferric oxide since the cation is Fe3 .

Table of Type II Compounds AC Traditional -ous Root -ic per (I) & copper (II) cupr- Cu Cu d (I) & gold (III) aur- Au Au3 cury (I) & mercury (II) mercur- Hg2 Hg 2 omium (II) & chromium (III) chrom- ganese (II) & manganese (III) mangan- n (II) & iron (III) ferr- alt (II) & cobalt (III) cobalt- Co2 kel(II) & nickel (III) nickel- Ni2 (II) & tin (IV) stann- d (II) & lead (IV) ium (III) & cerium (IV) Cr2 Cr3 Fe2 plumb- Fe3 Sn4 Pb2 Ce 2 Mn2 Sn2 cer- 2 Pb4 Ce4 3 enic (III) & arsenic (V) arsen- As3 As5 imony (III) & antimony (V) antimon- Sb3 Sb5 muth (III) & bismuth (V) bismuth- Bi3 Bi5

Rules for Naming Binary Covalent Compounds How do you recognize that something is a binary covalent compound (versus an ionic compound)? 1.) If a compound contains only nonmetals (no metals), then you can be reasonably sure that it is a covalent compound. Note: Some exceptions would be compounds that contain polyatomic ions. For example, ammonium bromide NH4Br and ammonium sulfate (NH4)2SO4 are ionic compounds even though they contain only nonmetals.

Type III Compounds: Binary Covalent Compounds 1.) The first element in the compound is named first using the name of the element. 2.) The second element is named as though it were an anion (the root name suffix ide); even though, we know there are no anions in a covalent compound. 3.) Prefixes are used to denote the numbers of each atom present. Since there are no formal charges on the atoms in covalent compounds, it is more difficult to predict the proportions that the atoms combine in. (Note: the prefix mono is never used with the first element).

Type III Compounds: Binary Covalent Examples of binary covalent compounds include water (H O), Compounds 2 carbon monoxide (CO), and carbon dioxide CO2. Prefix monoditritetrapentahexaheptaoctanonadeca- meaning one two three four five six seven eight nine ten The naming convention for binary covalent compounds is as follows: (prefix)-nonmetal (prefix)-nonmetal root "-ide. Try naming the compound P4O6.

Rules for Naming Simple Acids and Oxyacids How do we determine if something is an acid? The acids that we will be concerned with naming are really just a special class of ionic compounds where the cation is always H . Recall that cations are written first in ionic formulas. So if the formula has hydrogen written first, then this usually means that the hydrogen is an H cation and that the compound is an acid. When dissolved in water, acids produce H ions. These are also called protons, because when the electron is removed from a neutral hydrogen atom, it leaves behind one proton. If the counterion (the anion) to H in the acid is a polyatomic ion that contains oxygen (like NO2- or PO43-), the acid is called an oxyacid. If the anion

Binary acids are binary compounds that contain a hydrogen atom and either a halogen (F, Cl, Br, I) or sulfur (S). It is important to note that nitrogen, phosphorus, and oxygen do not form binary acids with hydrogen. The naming convention for binary acids is as follows: “Hydro-” nonmetal root “-ic” “acid” The nonmetal roots are determined as follows. For the halogens, simply remove the “ine” and for sulfur remove the “ur”. Thus, the roots for fluorine, chlorine, bromine and iodine are fluor-, chlor-, brom-, and iod- ; and for sulfur, sulf- . So to determine the name for HCl: hydro chlor ic acid acid hydrochloric If the acid is in a gaseous form or an anhydrous form, the "-ic" is replaced by "-ide" and the

So, acids are formed by adding protons to atoms or radicals with negative valence numbers. The names of acids that do not contain oxygen are formed like those of binary acids by adding the prefix hydro- to the root name for the element and adding the suffix –ic and the word “acid”. Formula Acid Name HF hydrofluoric acid HCl hydrochloric acid HBr hydrobromic acid HI hydriodic acid HCN hydrocyanic acid H 2S hydrosulfuric acid HN3 type of oxygen acid hydrazoic acid If only one is formed, then the name is that of the characteristic element plus the suffix –ic and the word acid. Formula Acid Name H3BO3 boric acid H2CO3 carbonic acid H4SiO4 silicic acid

Acids formed from polyatomic ions have a naming system similar to that of the polyatomic ions themselves. The difference being that for “-ate” we substitute “-ic” and for “-ite” we substitute “ous” and add the word acid. For example, hypochlor-ite then becomes hypochlorous acid; and perchlor-ate becomes perchloric acid. Ion Ion name Acid Formula Acid Name ClOhypochlorite HClO hypochlorous acid ClO2 chlorite HClO2 chlorous acid ClO3 chlorate HClO3 chloric acid The perchlorate number of hydrogens HClO added to the perchloric polyatomic ClONote: 4 4 ion is equal to the charge on the cation. acid Try naming the acids formed by nitrite and nitrate ions, NO2 – and NO3 -, respectively.

Organic Organic compounds contain Compounds carbon. All other compounds are defined as inorganic. However, for the sake of convenience, some carbon compounds are considered inorganic: carbon monoxide (CO), carbon dioxide (CO2), carbon disulfide (CS2), and those containing the anions: cyanide (CN-), carbonate (CO3 2-) bicarbonate (HCO3-)

Organic The alkanes consist only of carbon and hydrogen held together Compounds by single bonds. The first four alkanes have common names. The higher ones have names reflecting the Greek/Latin prefixes used in the covalent naming system. Organic Compounds Names CH4 methane C2H6 ethane C3H8 propane C4H10 butane C5H12 pentane C6H14 hexane C7H16 heptane C8H18 octane C9H20 nonane C10H22 decane The alkenes have a double bond between two of the carbons. Every double bonded carbon can only form two other bonds. So there are two less hydrogens for every corresponding alkene. The alkynes have a triple bond between two of the carbons. So every triple-bonded carbon can only form one other bond.

Listen here! Y’all know I Might Pass Maybe 0002 https://www.youtube.com/watch?v WRlGwnxs-pM Remember that “Ate Beats Ite!” and hydroxide! OH - istry Song (to the tune of I Will Follow You Into the Dark by Death Cab for s://www.youtube.com/watch?v pBxIGmlqr-s

For February 3-5 Read: The Statistical Analysis of Zinc Washers – Text Due: pp 53-76 Nomenclature – Packet pp 53-67 (pp 55-67 extra credit) Dimensional Analysis 1 – Text pp 15-24 Problems 1, 3, 8, 11, 14, 15, 17, 19, 20, 21 & 22 Do not apply rules of significant figures. Must show work to receive credit. Significant Figures – Text pp41-2 & 51-52 Problem Set 1 & 2 – Do all problems.