Call for Papers: 2nd ACM Special Interest Group on Health ...

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Call for Papers: 2nd ACM Special Interest Group on Health Informatics (SIGHIT) International Health Informatics Symposium (IHI 2011) Country: United States State: Florida Date: 5/23/2011 Call for Papers: 2nd ACM Special Interest Group on Health Informatics (SIGHIT) International Health Informatics Symposium (IHI 2011) 2nd ACM SIGHIT International Health Informatics Symposium November 9-11, 2011 Miami, Florida We cordially invite you to submit your contribution to the 2nd ACM SIGHIT International Health Informatics Symposium (IHI 2011).

• biomedical modeling
• usability studies
• health informatics
• clinical outcomes
• medical devices
• data mining
• healthcare
• systems
• data

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• Révision
• Exposé
• Computing
• Health care
• Health
• Médecine
• System

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• Publié par: nachig
• Nombre de lectures: 33
• Langue: English

Extrait

Lab Session 5, Experiment 4 Chemical Nomenclature Objective: To learn how to read and write formulas of compounds Background: Many of the substances you will encounter in this laboratory are ionic compounds. They are made up of ions which have an unequal number of protons and electrons. Ion is a charged species. If an element loses an electron, is it called at cation resulting in a positive charge. If an element gains an electron, is it called an anion resulting in a negative charge. Atoms of metals usually lose electrons. Atoms of nonmetals typically gain electrons. A polyatomic ion is a group of atoms that are bonded together and have an unequal number of protons and electrons. Ionic compound names are read by stating the name of the cation, followed by the name of the anion. The formulas are written as: x+ y- (cation) (anion) (cation) y (anion) x The subscripts (x and y) are the smallest possible whole numbers that would make the total charge equal to zero. If a subscript is 1, it is omitted. If the ion is a polyatomic ion and the subscript is not one, then parentheses are placed around the polyatomic ion’s formula before writing the subscript. The charges of the ions are not included in the formula of the compound. The charge of the ion is only written when the formula of the ion is written by itself. There are two situations of naming inorganic compounds. •group A metals are simple ionsGroup A metal and a nonmetal: 1.Just name the cation as its elemental name. 2.Just name the anion, changing the ending to –ide. AlCl 3 →aluminum chloride Li 2 S→lithium sulfide Ca 3 P 2 →calcium phosphide K 2 O→potassium oxide •Group B metal and a nonmetal: group B metals have changing charges 1.Determine charge on the cation 2.Name the cation 3.Place roman numeral after the cation to indicate its charge +1 = I +2 = II +3 = III +4 = IV +5 = V +6 = VI +7 = VII +8 = VIII +9 = IX +10 = X

4.Name the anion with an –ide ending. FeCl 2 →iron (II) chloride FeCl 3 →iron (III) chloride SnO 2 →tin (IV) oxide SnO→tin (II) oxide •With a polyatomic: 1.name the cation ion, and then name theWith a group A metal: polyatomic 2.With a group B metal: determine the charge, name the cation, use a roman numeral, and then name the polyatomic 3.name the cation, name the nonmetal anionWith a polyatomic cation: with –ide ending 4.With two polyatomics: just name each of them in order 2+ 1- Example: Ions: Ca and Cl  Formula: CaCl 2  Name: Calcium chloride + 2- Example: Ions: NH 4 and SO 4  Formula: (NH 4 ) 2 SO 4  Name: Ammonium sulfate Compounds composed of two nonmetals usually are not ionic, but covalent. Therefore, there are no ions, only atoms bonding together. Formulas of compounds such as these are written so that the subscripts (x and y) are whole numbers. If not specified, a subscript of 1 is implied. Use the following rules for naming binary compounds: 1.If MORE than one atom of the first element is present in the formula, state the prefix corresponding to that number. Do not use a prefix if there is only one atom present. 2.State the name of the first element. 3.Always state the prefix corresponding to the subscript of the second element (mono for one). 4.State the name of the root of the second element followed by the suffix –ide. 5.The following list includes the prefixes corresponding to the number of an element’s atoms present in the formula. mono = 1 hexa = 6 tetra = 4 nona = 9 di = 2 hepta = 7 penta = 5 deca = 10 tri = 3 octa = 8 Example: Formula: OF 2  Name: Oxygen difluoride Example: Formula: P 2 O 5  Name: diphoshorous pentoxide Example: Formula: CO  Name: carbon monoxide

List of polyatomic ions: - -2 Hydroxide Sulfite OH SO 3 + - Ammonium NH Hydrogen sulfate 4 HSO 4 - (or bisulfate) Nitrate NO - 3 Hydrogen sulfite - HSO 3 Nitrite NO (or bisulfite) 2 -3 - Phosphate Perchlorate PO ClO 4 4 -2 - Hydrogen  Chlorate HPO ClO 4 3 phosphate - Chlorite - ClO 2 Dihydrogen H PO 2 4 - Hypochlorite phosphate ClO -3 -2 Phosphite Carbonate PO CO 3 3 - - Permanganate Hydrogen MnO HCO 4 3 -2 carbonate (or Chromate CrO 4 bicarbonate) -2 Oxalate - C O Cyanide CN 2 4 -2 - Dichromate Acetate Cr O C H O (or 2 7 2 3 2 +2 - CH COO ) Mercury (I) Hg 3 2 -2 Sulfate SO 4 Experimental procedure: 1.Group 1A metal atoms tend to lose 1 electron and become a cation with a charge of 1+. Typically, so does silver (Ag). Write the formulas of the ions provided on the data summary sheet. 2.Group 2A metal atoms tend to lose 2 electrons and become a cation with a charge of 2+. Typically, so does zinc (Zn) and cadmium (Cd). Write the formulas of the ions provided on the data summary sheet. 3.Group 3A metal atoms tend to lose 3 electrons and become a cation with a charge of 3+. Write the formulas of the ions provided on the data summary sheet. 4.Transition metal atoms may lose a variable number of electrons, depending on the reaction condition. Also some of the larger representative metals can form more than one cation. If two or more charges are possible, it is necessary to specify the charge by using a roman numeral in parenthesis after stating the name of the cation. Write the formulas of the ions provided on the data summary sheet. 5.Atoms of the nonmetals in Group 7A (the halogens) tend to gain one electron and become anions with a charge of 1-. The name of an anion is composed of the root of the nonmetal’s name and the suffix –ide. Write the formulas of the ions provided on the data summary sheet. 6.Atoms of nonmetals in Group 6A tend to gain two electrons and become anions with a charge of 2-. The name of the anions is composed of the root of the nonmetal’s name and the end with a suffix of –ide. Write the formulas of the ions provided on the data summary sheet.

7.On the answer sheet write the correct formula for the ionic compounds. 8.On the answer sheet write the name of the ionic compounds. For the compounds containing metals that can form more than one cation, be sure to include roman numerals. 9.On the answer sheet name the binary compounds composed of nonmetals. 10.On the answer sheet write down the correct formula for the binary compounds composed of nonmetals. Naming Compounds Flow Chart

Is a polyatomic present?

Rules 1. Name the cation. 2. Use Roman numerals only if transition metal is present. 3. Just name the polyatomic anion. 4. Use parenthesis is more than one if present. 5. Use no prefixes.

no

Is the compound binary?

Rules 1. Name the first element as a cation. 2. Name the second element as anion (ide ending). 3. ALWAYS use prefixes on the anion. 4. Use prefixes on cation only if more than one is present. 5. Use no roman numerals.

no

yes

Does it contain a metal?

no

yes

Is it a transition metal?

Rules 1. Just name the cation. 2. Name the anion (ide ending). 3. Use no prefixes 4. Use no roman numerals. +1 5. Includes Ag , +2 +2 Zn , Cd 6. Excludes In, Sn, Pb, Tl, Bi

yes

Rules 1. Determine charge on cation. 2. Name the cation. 3. Specify the charge on the cation with roman numerals. 4. Name the anion ( ide ending). 5. Use no prefixes. +1 6. Excludes Ag , +2 +2 Zn , Cd 7. Includes In, Sn, Pb, Tl, Bi

NOTES

NOTES

t)Copper (II) ion

e)Oxide ion

__________

__________

l)Strontium ion

__________

__________

__________

__________

b)Lithium ion

e)Rubidium ion

c)Potassium ion

a)Sodium ion

a)Fluoride ion

d)Iodide ion

j)Zinc ion

i)Beryllium ion

f)Silver ion

c)Chloride ion

__________

__________

__________

Lab Session 5, Experiment 4 Chemical Nomenclature Name: _______________________________________ Date: ________________________________________ Instructor: ____________________________________ DATA SUMMARY SHEET CHEMICAL NOMENCLATURE Cations:

p)Iron (III) ion

__________

m)Cadmium ion

__________

__________

n)Aluminum ion

__________

__________

__________

__________

__________

__________

f)Selenide ion

__________

q)Tin (II) ion

d)Cesium ion

o)Iron (II) ion

__________

s)Copper (I) ion

__________

__________

__________

h)Telluride ion

__________

__________

__________

g)Sulfide ion

__________

v)Lead (IV) ion

u)Lead (II) ion

r)Tin (IV) ion

h)Barium ion

__________

__________

g)Magnesium ion

Anions:

k)Calcium ion

__________

b)Bromide ion

p)Magnesium hydroxide

r)Lithium hydroxide

o)Cadmium fluoride

n)Ammonium phosphate

q)Rubidium sulfate

u)Zinc sulfate

_________________________________

_________________________________

_________________________________

b)Tin (IV) hydroxide

a)Silver Selenide

c)Potassium sulfate

d)Lithium sulfate

_________________________________

_________________________________

g)Magnesium carbonate

_________________________________

_________________________________

v)Lead (II) acetate

s)Mercury (II) oxide

l)Zinc chloride

h)Cobalt (II) bromide

e)Ammonium sulfate

i)Sodium oxide

f)Barium carbonate

t)Aluminum permanganate

_________________________________

_________________________________

_________________________________

_________________________________

_________________________________

_________________________________

_________________________________

_________________________________

Write the correct formula for the ionic compounds.

_________________________________

_________________________________

_________________________________

_________________________________

_________________________________

k)Aluminum iodide

j)Barium bromide

_________________________________

m)Silver phosphate

_________________________________

_____________________________________________

_____________________________________________

_____________________________________________

_____________________________________________

_________________________________

c)Na 2 CO 3

f)Zn 3 (PO 4 ) 2

_________________________________

_________________________________

g)BaBr 2

h)AgCl

i)CaSO 4

j)MgSO 3

h)Sodium bicarbonate

f)Cobalt (II) hydroxide

b)Magnesium chloride

_________________________________

g)Ammonium sulfide

_____________________________________________

a)Sodium chloride

e)Tin (IV) oxide

c)Mercury (II) nitrate

d)Zinc nitrate

_________________________________

b)CaCl 2

k)Aluminum dichromate

i)Tin (II) phosphate

j)Iron (II) sulfide

_____________________________________________

_____________________________________________

_________________________________

_________________________________

_____________________________________________

d)Fe(NO 2 ) 3

e)Fe(NO 3 ) 2

_________________________________

_________________________________

_________________________________

_________________________________

_____________________________________________

Write the name of the ionic compounds. For the compounds containing metals that can form more than one cation, be sure to include roman numerals. a)K 2 S _____________________________________________

_____________________________________________

Name the covalent compounds composed of nonmetals.

_________________________________

a)CF 4

_____________________________________________

_____________________________________________

_____________________________________________

b)Carbon tetrachloride

c)Carbon dioxide

d)Dinitrogen trioxide

g)NO

_____________________________________________

_____________________________________________

_____________________________________________

e)SO 3

m)Na 2 SO 4

n)K 3 PO 3

_________________________________

_________________________________

_____________________________________________

d)S 2 F 2

c)SF 6

_____________________________________________

f)Another name for dihydrogen monoxide is: ______________________

e)Dihydrogen monoxide

_____________________________________________

_________________________________

_____________________________________________

b)P 4 O 10

k)Sn 3 (PO 4 ) 4

_________________________________

a)Phosphorous pentachloride

Write down the correct formula for the covalent compounds composed of nonmetals.

f)PCl 3

o)Cu(NO 3 ) 2

l)NaBr

_____________________________________________