Writing Formulas and Names of Compounds

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1 Writing Formulas and Names of Compounds PURPOSE - Determine the charge of an ion by observing its electron dot structure. - Write a correct formula and name of an ionic compound. - Determine the number of covalent bonds needed by non metal elements. - Write correct formulas and names for covalent compounds. MATERIALS - paper - pencil DISCUSSION When we consider the chemical reactivity of elements, we are primarily interested in the electrons in the highest energy level called the valence electrons. The octet rule tells us that atoms are most stable when they have eight electrons in the valence shell. The exceptions are the elements H and He which are stable with two electrons.

2 PART I: IONIC CHARGES When atoms in groups IA, IIA, or IIIA react with atoms in groups VA, VIA, and VIIA, they form stable octets in their valence shells by losing or gaining electrons. We can predict what this loss or gain is by observing the initial electron dot structures. An electron dot structure is written by placing dots that represent valence electrons around the symbol of the atom. Aluminum, for example, whose electron configuration is 2, 8, 3 has three valence electrons and an electron dot structure of The aluminum atom loses its three valence electrons to become stable. The resulting aluminum ion has an electrical charge or valence of 3+ and an electron configuration of 2, 8 which is stable. Al atom Al 3+ ion 13 p+ 13 p+ 13e- 10e- 0 charge 3+ charge Elements (metals) with one, two or three valence electrons LOSE their valence electrons to form positively charged ions. Elements (nonmetals) with five, six, or seven valence electrons GAIN electrons to become stable and form negatively charged ions. Complete the chart of the dot structures and state their resulting ionic charges and names. The positive ions are named just like the element. The negative ions are named by changing the ending of the elemental name to ide. Element Atomic number e- arrangement (atom) Dot formula Loss or gain e- e- arrangement (ion) Charge (ion) Ion Name of ion Sodium 11 2,8,1 Na. Lose 1e 2,8 1+ Na + Sodium Oxygen Chlorine Aluminum Fluorine Potassium Sulfur Magnesium

3 PART II: WRITING IONIC FORMULAS An ionic formula represents the smallest number of positive ions and negative ions that give a charge balance of zero. Below indicate the number of each ion needed to give an overall charge balance. Write the correct formula with the number of each ion needed as a subscript. The compound is named by writing the name of the positive ion followed by the name of the negative ion. Ions # for charge balance formula name Ca 2+ 1 needed CaCl 2 calcium chloride 2 needed Na + Na + O 2- Na + N 3- Mg 2+ Mg 2+ O 2- Mg 2+ N 3- Al 3+ Al 3+ O 2- Al 3+ N 3-

4 PART III: VARIABLE VALENCES FOR TRANSITION METALS Many of the transition metals are capable of forming ions with more than one type of positive valence. Below are examples with iron and copper. The names include the particular valence in parentheses following the name of the metal. Complete the formulas and names of the following compounds. Fe 2+ iron(ii) or ferrous ion Fe 3+ iron(iii) or ferric ion Cu + copper(i) or cuprous ion Cu 2+ copper(ii) or cupric ion Ions number needed Formula Name Fe 2+ 1 needed FeCl 2 iron(ii) chloride 2 needed Fe 2+ Br - Cu 2+ F - Fe 3+ S 2- Cu + P 3-

5 PART IV: POLYATOMIC IONS Polyatomic ions are groups of atoms chemically combined with an overall charge, usually negative. A list of several polyatomic ions is located on your periodic table. Note that the endings of the polyatomic ions are different; they typically end with ate or ite. Below is an example of an ionic compound with a polyatomic ion. When more than one polyatomic ion is needed to complete the charge balance, parenthesis are used to surround the entire ion while the subscript needed to balance the charge is on the outside. No change is made in the formula of the polyatomic ion itself. Ions number needed Formula Name Ca 2+ 1 needed Ca(NO 3 ) 2 calcium nitrate NO 3-2 needed Mg 2+ NO 2 - Na + SO 4 2- Fe 2+ PO 4 3- Ca 2+ HCO 3 -

6 PART V: COVALENT (MOLECULAR) COMPOUNDS Two different nonmetals form a compound by sharing electrons. The resulting compound has covalent bonds and is called a covalent compound. To write the formula of a covalent compound, you need to determine the number of electrons needed by each kind of atom to provide an octet. Nitrogen for example has five valence electrons. Nitrogen atoms need three more electrons for an octet; they also share three electrons. Complete the following table. Element Electron Dot Structure Electrons to Share C 4 N O Cl H P S PART VI: WRITING FORMULA OF COVALENT COMPOUNDS Formulas of covalent compounds are derived by sharing the valence electrons of the atoms until ach atom acquires an octet (except H and He which fill with just two electrons). Write the correct formulas for the following pairs of elements. Element Electron Dot Structure Formula C and H CH 4 N and H H and Cl H and H Cl and Cl P and Cl

7 PART VII: MIXED PRACTICE Write the correct formulas for the following compounds: sodium oxide iron (III) sulfate magnesium fluoride nitrogen tribromide copper(ii) chloride sodium carbonate iron(ii) bromide copper (I) oxide aluminum nitrate aluminum chloride carbon tetrachloride potassium iodide Write the correct name of the following compounds: CuO N 2 O 4 Al(NO 3 ) 3 Ag 2 O FeCO 3 Na 2 S Cu(OH) 2 PCl 3 Your friend wants to know what the formula FeSO 4 on her vitamin bottle means and what its name is. What would you tell her?

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