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Chemical Names and Formula

Chemical Names and Formula. Chemistry Cook. Periodic Table. There are over 90 naturally occurring elements/atoms and about 25 elements made in the lab. Various combinations of atoms can be formed, and which such diversity we need a way to name and communicate these variations. Periodic table.

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Chemical Names and Formula

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  1. Chemical Names and Formula Chemistry Cook

  2. Periodic Table • There are over 90 naturally occurring elements/atoms and about 25 elements made in the lab. • Various combinations of atoms can be formed, and which such diversity we need a way to name and communicate these variations

  3. Periodic table • Elements are arranged in row and columns on the: Periodic table • Hydrogen, the smallest and lightest element in top right corner • Helium is atomic number 2

  4. Atomic Numbers • Krypton

  5. Calculate • For any element: • Number of Protons = Atomic Number • Number of Electrons = Number of Protons = Atomic Number • Number of Neutrons = Mass Number - Atomic Number • For krypton: Number of Protons = Atomic Number = 36 • Number of Electrons = Number of Protons = Atomic Number = 36 • Number of Neutrons = Mass Number - Atomic Number = 84 - 36 = 48

  6. Periodic Table • A column of elements in the periodic table is known as a group • There are 18 groups • Group 1A: • H • Li • Na • K • RB • Cs

  7. Breakdown of each group • Group 1=Alkali Metals • Group 2= Alkaline Earth Metals • Group 3-12= Transition metals • Group 13,14 & 15= Other metals • Metalloids=Boron diagonal down over and down over( A big L) • Group 14-16 =Non Metals • Group 17= Halogens (salt formers) • Group 18= Noble gases • Rare Earth Metals= Man made elements inserted in the transition metal at 56 and 88 • Chemical Elements.com - Noble Gases

  8. Alkali Metals/Representative metals (A) • The illustrate the entire range of chemical properties • Both metals and non metals • They do not include transition metals or inner transition metals (man made ones)

  9. Metallic Metals • A Groups (1, 2 13-18) • Have high luster when cleaned • High electrical conductivity • Ductile • Can be drawn into wires • Malleable • Beaten into sheets (dyes at GM plants)

  10. Groups • 1A starts with H or Li • Hydrogen is special It is a non metal in group 1A • 2A starts with Be • 3A starts with B • 4A starts with C • 5A starts with N • 6A starts with O • 7A starts with F

  11. Transition Metals (B) • B group elements • Inner transition metals (rare earth metals).

  12. Non Metallic • Elements that are: • Non lustrous • Poor conductors of electricity • Some are gases • Others are brittle solids and some liquids at room temperature

  13. Semi Metals or Metalloids • Elements with the properties of both metals and nonmetals • Silicon • Found in transistors • Good semi conductor • Conducts electricity in a special way • Breast implants (cheap ones)

  14. Atoms and Ions • All elements are composed of atoms of the same kind • Atomic Theory (review) • An atom is electrically neutral because it has an equal number of protons and electrons • Na atomic number is 11 and has 11 protons and is positively charged, has 12 neutrons • Because Neutrons have no charge the total charge of Na is (+11)+ (11)=0 • When elements form compounds they can gain or lose electrons, and when the number of electrons is not equal to the number of protons then the atom becomes a • Ion

  15. IOns • Are atoms or groups of atoms that have a positive or negative charge • Formed when atoms gain or lose electrons

  16. Positive ions • Metals tend to form positive ions by losing one or more electrons • Cation • Any atom or group of atoms with a positive charge • Na ion is form by the loss of one electron from the Na atom • Sodium ion has 11 protons and 10 electrons it has a charge of 1+ • Atomic charges are written with the number followed by a sign • Na1+ or Na+ (always write ions this way) • If the number is 1 it can be omitted

  17. Ions • Mg ions are formed differently because they have different valence electrons (electrons in outer shell) • Mg has a charge of 2+ so it has 12 protons, and 10 electrons

  18. Negative Ions • Nonmetallic elements tend to gain one or more electrons • Anions • Atoms or groups of atoms with a negative charge • Anions have more electrons (unlike cations). • Cl ions has 17 protons and 18 electrons • It has a charge of -1 • Oxide ion has a charge of -2

  19. Compounds • Are pure substances the differ from elements because they contain more than one kind of atom. • Law Of Definite Proportions: In any chemical compound the elements are always combined in the same proportion by mass • A Molecule is a neutral group of atoms that act as a unit. All molecules of a given compound are neutral. • Compounds that are composed of molecules are molecular compounds.

  20. Law of Definite Proportions • MgS is a compound. IF we have 100g of this compound • It will always contain: • 43.13g of Mg • 56.87g of S • This mass ratio will never change no matter how much you have

  21. Chemical Formulas • There are more than 4 million chemical compounds. • Chemical Formulas • Some are molecular • Some are ionic • A chemical formula shows the number and kinds of atoms present in a molecule. • A molecular formula shows the number and kinds of atoms present in a molecule of a compound • Example = H2O CO2 C2H6 C2H6O

  22. Formulas and Names of Common Metals Ions with more than 1 ionic charge • Formula NameStock NameClassical Name • Cu1+ Copper (I) Ion Cuprious ion • Cu2+ Copper (II) Ion Cupric Ion • Fe2+ Iron (II) Ion Ferrous Ion • Fe3+ Iron (III) Ion Ferric Ion • Hg2 Mercury (I) Ion Mercurrous Ion • Hg2+ Mercury (II) Ion Mercuric Ion • Review Table 5-3

  23. Rules for naming • Compounds that give OH- ions • Bases • Compounds that give H+ ions • Acids • ite ending • Will always indicate less oxygen • ate ending • Will always indicate more oxygens

  24. Binary ionic compounds • Composed of two elements • Always cation and anion • They always have ide ending • Name metal first then put ide ending on nonmetal • Sodium chloride • Monoatomic always have ide ending

  25. Binary Ionic compounds • Name by writing name of cation followed by name of anion (ide ending).

  26. Ternary Ionic Compounds • Contain 3 different elements • They usually contain one or more polyatomic ions • First write down formulas of ions • Then balance charges • An ate or ite ending on polyatomic ion • Calcium nitrate

  27. Acids • Are compounds that give off hydrogen ions when dissolved in water. • When anion ends in ide the acid name begins with prefix hydro. The stem (nonmetal in most cases ends with ic) • HCl= hydrochloric acid

  28. rules

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