How Big Are Atoms? Five-hundred-million gold atoms lined up side-byside would form a line as long as a $10 bill.
Look around your home and you ll be amazed at the variety of chemicals in your cupboards and on your shelves. In the bathroom, you ll find water, soap, shampoo, and toothpaste - all chemicals. In the basement or garage, you may find cleaning products, such as ammonia and bleach, and perhaps painting and gardening products. In your kitchen, you ll likely find table salt, baking soda, and baking powder. Each of these compounds has a chemical name and a chemical formula. The formula identifies which elements, and how much of each, are in the compound. So, for example, table salt s chemical name is sodium chloride and its formula is NaCl. Baking soda s chemical name is sodium bicarbonate and its chemical formula is Na(HCO 3 ).
NAMING CHEMICAL COMPOUNDS Until the 18th century, no standardized system existed for naming chemicals. This created confusion because the names for chemical compounds varied from country to country and scientist to scientist. For example, hydrochloric acid and muriatic acid refer to the same thing. If you didn t know that, you might think they were two different chemicals. Today, some compounds are better known by their common name. Bleach, for instance, is almost always used instead of the chemical name aqueous sodium hypochlorite. In 1787, a French chemist named Guyton de Morveau created a naming system, or nomenclature, for compounds. He decided to use the chemical name for each element in the compound, always putting the metal element first. For example, zinc and oxygen combine to form zinc oxide. Since 1920, the International Union of Pure and Applied Chemistry (IUPAC) has been the body responsible for agreeing on the appropriate name for every chemical compound discovered.
INTERPRETING CHEMICAL NAMES AND FORMULAS FROM COMPOUNDS If you know only the formula of a chemical compound, you can determine its chemical name. If you know only its name, you can determine its formula. Table salt s chemical name, sodium chloride, indicates that the compound is made of one atom of sodium and one atom of chlorine Its chemical formula, NaCl, indicates this too. One sodium atom combines with one chlorine atom to form the compound sodium chloride, which we call table salt
Now look at the formula for the compound water: H 2 O. Notice that next to the H is a small 2 as a subscript. ( Sub means below.) The 2 indicates that there are two atoms of hydrogen to go with every atom of oxygen in water. Subscript numbers in a chemical formula indicate the number of atoms of the elements that must combine to form the compound. No subscript number indicates that only one atom of that element is needed. In water, two hydrogen atoms join with each oxygen atom.
Compound Chemical Formula Elements No. of Atoms of Each Total No. of Atoms sodium chloride NaCl sodium chlorine 1 1 2 water H 2 0 hydrogen oxygen 2 1 3
INDICATING THE PHYSICAL STATE OF A COMPOUND Another common notation added to chemical compounds indicates the state of the chemical at room temperature. After the chemical formula, a subscript s for solid, l for liquid, or g for gas is shown in parentheses. For example, sodium chloride is written as NaCl ( s), water is written as H 2 O (l), and natural gas (methane) is written as CH 4 (g). For aqueous solutions (substances dissolved in water), a subscript aq in parentheses is added to the formula. So, if sodium chloride was dissolved in water, the resulting aqueous solution would be written as NaCl (aq).
Glucose C 6 H 12 O 6 (s) The chemical formula for glucose tells us that each molecule is made of 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms and the (s) indicates it is a solid. 24 atoms in all.
Common Name: Peroxide Scientific name : Hydrogen peroxide Chemical Formula: H 2 O 2 (aq) Number of Elements: 2 Hydrogen, Oxygen Number of Atoms of each element: Hydrogen- 2 Oxygen- 2 2 elements 4 atoms
Common Name: Sugar Scientific name : sucrose Chemical Formula: C 12 H 22 O 11 (s) Number of Elements: 3 Carbon, Hydrogen, Oxygen Number of Atoms of each element: Carbon-12 Hydrogen- 22 Oxygen- 11 3 elements 45 atoms
Common Name: Baking soda Scientific name : sodium hydrogen carbonate Chemical Formula: NaH(CO 3 ) (s) Number of Elements: 4 Sodium, Hydrogen, Carbon, Oxygen Number of Atoms of each element: Sodium - 1 Hydrogen - 1 Carbon -1 Oxygen - 3 4 elements 6 atoms
Common Name: Rubbing alcohol Scientific name : 2-propanol Chemical Formula: CH 3 CH(OH)CH 3 (l) Number of Elements: 3 Carbon, Hydrogen, Oxygen Number of Atoms of each element: Carbon-3 Hydrogen- 8 Oxygen- 1 3 elements 12 atoms
Common Name: Aspartame Scientific name : aspartyl-phenylalanine methyl ester Chemical Formula: C 14 H 18 N 2 O 5 (s) Number of Elements: 4 Carbon, Hydrogen, Nitrogen, Oxygen Number of Atoms of each element: Carbon-14 Hydrogen- 18 Nitrogen- 2 Oxygen- 5 4 elements 39 atoms
Common Name: Milk of Magnesia Scientific name : Magnesium Hydroxide Chemical Formula: Mg(OH) 2(s) Number of Elements: 3 - Magnesium, Oxygen, Hydrogen Number of Atoms of each element: 1 - Mg, 2- Oxygen, 2- Hydrogen 3 elements 5 atoms
Common Name: Citric acid Scientific name : 2-hydroxy-1,2,3- propanetricarboxylic acid Chemical Formula: C 3 H 4 (OH)(COOH) 3 (s) Number of Elements: 3 - Carbon, Hydrogen, Oxygen, Number of Atoms of each element: Carbon - 6, Oxygen - 7, Hydrogen - 8 3 elements 21 atoms
Sodium, shown in (a), is a metal. Sodium combines with chlorine gas in a violent reaction (b). The product is table salt, NaCl (s) (c). Na + Cl 2 NaCl 2 Na + Cl 2 2 NaCl
Sodium chloride is called an ionic compound. Ionic compounds are pure substances formed as a result of the attraction between particles of opposite charges, called ions. Table salt is formed from positively charged sodium ions and negatively charged chloride ions. Other properties of ionic compounds include: their high melting point, good electrical conductivity, and distinct crystal shape. All ionic compounds are solids at room temperature. In fact, table salt will not melt until it is heated to 801 C. When an ionic compound is melted or dissolved in water, it will conduct electricity. This property of ionic compounds led to the study of electrochemical cells (cells that either convert chemical energy into electrical energy or electrical energy into chemical energy). And that work in turn eventually led to the invention of batteries. Ion Origin The word ion comes from a Greek word meaning to go or wander.
When the ionic compound is dissolved in water, the metal and nonmetal form an aqueous solution of ions. An ion is an atom or a group of atoms that has become electrically charged through the loss or gain of electrons. The following table shows some examples of ion charges for various elements.
Sodium - Na Chlorine Cl Sodium Ion charge 1 + Sodium will lose 1 electron Sodium has 1 valence electron Think of it as being able to fill in 1 hole. Chlorine Ion charge 1 Chlorine gain 1 electrons Chlorine has 7 valence electrons Think of it as having 1 hole.
The crystals in this table salt are held together by ionic bonds.
Ion Charges To indicate ions in written notation, a plus sign (+) or a minus sign (-) is placed to the upper right of the element symbol. This is a superscript position (super - means above ). For example, a sodium ion is written as Na + and a chlorine ion as Cl -. Naming Ionic Compounds 1. The chemical name of the metal or positive ion goes first, followed by the name of the non-metal or negative ion. 2. The name of the non-metal negative ion changes its ending to ide.
Hydrogen Hydride Nitrogen - Nitride Phosphorus Phosphide Oxygen Oxide Sulfur Sulfide Selenium Selenide Fluorine Fluoride Chlorine Chloride Bromine - Bromide Iodine - Iodide
Lithium Fluoride Li F Lithium 1 + has 1 extra valence electron can fill one hole Fluorine 1 - missing 1 valence electron has one hole 2. Lithium + Oxygen Lithium Oxide Li 2 O Lithium 1 + has 1 extra valence electron can fill one hole Oxygen 2 - missing 2 valence electrons has two holes Lithium 1 + can fill one hole you need 2 Li atoms to fill 2 holes 2. Lithium + Nitrogen Lithium Nitride Li 3 N Lithium 1 + has 1 extra valence electron can fill one hole Nitrogen 3 - missing 3 valence electrons has three holes Lithium 1 + can fill one hole you need 3 Li atoms to fill 3 holes
4 5 6 7 8 9 10 Sodium Chloride Sodium Sulfide Sodium Nitride Sodium Phosphide Potassium Bromide Potassium Sulfide Potassium Nitride NaCl Na 2 S Na 3 N Na 3 P KBr K 2 S K 3 N 11 Beryllium Iodide Bel 2 12 Beryllium Oxide BeO 13 Beryllium Nitride Be 3 N 2
14 Calcium Fluoride CaF 2 15 Calcium Oxide CaO 16 17 Calcium Phosphide Ca 3 P 2 Magnesium Iodide MgI 2 18 Magnesium Sulfide MgS 19 20 Magnesium Nitride Mg 3 N 2 Magnesium Chloride MgCl 2
Metals that have more than 1 ionic charge Some elements with more than one ion charge: Titanium 3 + or 4 + Iron 3 + or 2 + Nickel 2 + or 3 + Copper 1 + or 2 + Lead 2 + or 4 + Gold 1 + or 3 + Mercury 1 + or 2 + Use Roman Numerals to indicate the charge used I, II, III, IV, V, VI, VII, VIII
Titanium 3 + or 4 +, Iron 3 + or 2 +, Nickel 2 + or 3 +, Copper 1 + or 2 +, Lead 2 + or 4 + Gold 1 + or 3 +, Mercury 1 + or 2 + Roman Numerals to indicate the charge used (1) I, (2)II, (3)III, (4)IV, (5)V, (6)VI, (7)VII, (8)VIII 1.Titanium III Fluoride Ti F Ti 3+ F 1-3 One atom of titanium will fill 3 holes One atom of fluorine will has 1 hole to fill Titanium IV Fluoride Ti F Ti 4+ F 1-4 One atom of titanium will fill 4 holes One atom of fluorine will has 1 hole to fill 2.Titanium IV Oxide One atom of titanium will fill 4 holes One atom of oxygen will has 2 holes to fill Ti 3 + O 2 - Ti 4+ O 2- Ti O 2 Titanium III Oxide Ti 3+ O 2- One atom of titanium will fill 3 holes One atom of oxygen will has 2 holes to fill Ti O
3. Titanium III Nitride Ti N. Titanium IV Nitride Ti 3 N 4 4. Iron III Chloride Iron II Chloride 5. Iron III Sulfide Iron II Sulfide 6. Copper I Oxide Copper II Oxide FeCl 3 FeCl 2 Fe 2 S 3 FeS Cu 2 O CuO
8. Lead II Fluoride Lead IV Oxide 9. Gold I Oxide Gold III Nitride 10. Mercury I Oxide Mercury II Nitride Pb F 2 PbO 2 Au 2 O AuN Hg 2 O Hg 3 N 2
Polyatomic Ions Some ions can also form when certain atoms of elements combine. These ions are called polyatomic ions (poly - means many ). Polyatomic ions are a group of atoms acting as one. The formula is written in brackets. The name will not end in ide. Ammonium (NH 4 ) 1+ Bicarbonate (HCO 3 ) 1- Hydroxide (OH) 1- Nitrate (NO 3 ) 1- Nitrite (NO 2 ) 1- Carbonate (CO 3 ) 2- Sulfate (SO 4 ) 2- Sulfite (SO 3 ) 2- Phosphate (PO 4 ) 3-
Polyatomic Ions Cations (+1 Charge) Ammonium (NH 4 ) +
Polyatomic Ions Anions (-1 Charge) Bicarbonate (HCO 3 ) -
Polyatomic Ions Anions (-1 Charge) Hydroxide (OH) -
Polyatomic Ions Anions (-1 Charge) Nitrate (NO 3 ) - Nitrite (NO 2 ) -
Polyatomic Ions Anions (-2 Charge) Carbonate (CO 3 ) 2-
Polyatomic Ions Sulfate (SO 4 ) 2- Anions (-2 Charge) Sulfite (SO 3 ) 2-
Polyatomic Ions Anions (-3 Charge) Phosphate (PO 4 ) 3-
1. Ammonium + Fluorine 2. Ammonium + Oxygen 3. Ammonium + Nitrogen 4. Sodium + Hydroxide Ammonium Fluoride (NH 4 )F Ammonium Oxide (NH 4 ) 2 O Ammonium Nitride (NH 4 ) 3 N Sodium Hydroxide Na(OH) 5. Magnesium + Hydroxide Magnesium Hydroxide Mg(OH) 2
6. Calcium + Nitrate Calcium Nitrate 7. Potassium + Nitrite 8. Lithium + Carbonate 9. Potassium + Sulfite 10. Calcium + Phosphate Ca(NO 3 ) 2 Potassium Nitrite K(NO 2 ) Lithium Carbonate LI 2 (CO 3 ) Potassium Sulfite K 2 (SO 3 ) Calcium Phosphate Ca 3 (PO 4 ) 2
11. (NH 4 ) 2 O Ammonium Oxide 12. Ca (OH) 2 Calcium Hydroxide 13. K 2 (SO 4 ) Potassium Sulphate 14. K 3 (PO 4 ) Potassium Phosphate 15. Be (OH) 2 Beryllium Hydroxide
Bonus Metals with more than 1 charge 16. Cu(OH) 2 Copper II Hydroxide 17. Fe 2 (SO 4 ) 3 Iron III Sulfate 18. Hg 3 (PO 4 ) 2 Mercury II Phosphate 19. Pb(OH) 2 Lead II Hydroxide
When non-metals combine, a pure substance called a molecule or a molecular compound is formed. Molecular compounds differ from ionic compounds in several ways. They can be solids, liquids, or gases at room temperature. They tend to be insulators, or poor conductors of electricity. They also have relatively low melting and boiling points because the forces between the molecules are weak. Examples of molecular compounds: sugar, acetylene, and water.
Scientists have discovered more than 10 million compounds. At least 9 million are molecular compounds containing the element carbon.
WRITING FORMULAS FOR MOLECULAR COMPOUNDS Writing formulas for molecular compounds is similar to writing formulas for ionic compounds, except that no ions are present and the ion charge is not used in the formulas. This makes it hard to predict how non-metals combine. However, the formulas still clearly show what elements are present, and how many of each type of atom make up the molecule. For example, hydrogen gas is usually found as H 2. Each molecule has two atoms of hydrogen connected to each other. For ammonia ( NH 3(g) ), the situation is similar. Three hydrogen atoms combine with the nitrogen atom.
Naming of Molecular Compounds Non-metal + Non-metal 1. The first element in the compound uses the element name (just like the ionic compounds do). 2. The second element has a suffix ide (like the ionic compounds). 3. A prefix is used which tells how many atoms there are. 4. Exception to #3 above when the first element has only 1 atom the prefix mono is not used. Examples: CO 2 carbon dioxide CO carbon monoxide CCl 4 carbon tetrachloride H 2 O Dihydrogen monoxide
Number of Atoms Prefix 1 mono 2 di 3 tri 4 tetra 5 penta 6 hexa 7 hepta 8 octa 9 nona 10 deca
Molecular Compounds Non-metal + Non-metal CO 2 Carbon dioxide N 2 O Dinitrogen monoxide N 2 O 3 Dinitrogen trioxide NF 3 Nitrogen trifluoride CCl 4 Carbon tetrachloride PF 5 Phosphorus pentafluoride
a. disulfur tetrafluoride b. carbon trioxide c. nitrogen pentoxide d. nitrogen tribromide S 2 F 4 CO 3 NO 5 NBr 3 e. dinitrogen heptachloride N 2 Cl 7 f. carbon tetrachloride g. hydrogen monochloride CCl 4 HCl h. trihydrogen monophosphide H 3 P i. dihydrogen monoxide H 2 O
Comparing Ionic And Molecular Compounds