CHM 111 Lecture Notes - Lecture 17: Chemical Formula, Ionic Compound, Molar Mass

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30 Aug 2018

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CHM 111 Full Course Notes

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Subscripts specify the exact number of atoms of each element in one molecule of a covalent. Molecular formulae substance: ex: carbon dioxide (co2): 1 atom of carbon (cid:403) Ionic compounds, however, are written in formula units. As a result, the exact number of atoms of each element in the compound is not important. The formula unit is the smallest, electrically neutral collection of ions in an ionic compound. Thus, an ionic compound formula shows the simplest whole number ratio of atoms in the compound: ex: sodium chloride (nacl) is composed of one na+ for every cl-. Aluminum sulfide (al2s3) has 2 al+ for every three s- (cid:403) (cid:403) empirical formulae. Subscripts indicate relative number of atoms of each element in the molecule: ex: empirical formula for glucose: ch2o. Recall that molecules have formulas that specify the exact number of atoms of each element in one molecule of the substance.

Related Questions

1) How many atoms are there in 51.3 g of barium chloride (BaCl2)?
2) How many moles of carbon monoxide (CO) are in 29.3 g of the compound?

3) What is the formula for copper(II) phosphate? Capitalization and punctuation count?

4) How many atoms of phosphorus are in 2.90 mol of copper(II) phosphate?

5) How many moles of N are in 0.191 g of N2O?

6) A sample of C3H8 has 7.68 Ã 1024 H atoms. How many carbon atoms does the sample contain? What is the total mass of the sample?

7) Calculate the percent composition by mass of each element in Al(OH)3. Use at least three significant figures.

% Al= ?, % O=? , % H =?

8) What is the empirical formula of a compound composed of 3.25% hydrogen (H), 19.36% carbon (C), and 77.39% oxygen (O) by mass?

HCO (Insert subscripts as needed.)

9) A compound with the empirical formula CH2 has a molar mass of 98 g/mol. What is the molecular formula for this compound?

13%â¡ 8:08 PM ì docs.google.com Covalent Bonding and lonic Bonding study guide T-Mobile LTE Noteâ compare and contrast does not mean state one similarity and one difference Go back to our thinking maps and metacognitive logs and review everything we learned. Differentiate between the following: Atom, element, compound, bond, electron. Click here for a short video 2 Compare and contrast ionic and covalent bonds including the nature of the bonds. Click here for a video comparing the 2. Click here for a video on covalent bonding. s Explain the rules used for naming ionic compounds as well as those used for naming molecular compounds. You can either create 2 lists or 1 double bubble. 4 Use the periodic table to indicate whether the following molecules are ionic or covalent. Work each problem using either the diagram for transfer or sharing, then write the chemical formula and finally name each compound correctly. a NaBr b. HF d H20 s Explain why all of the following compounds will be molecular, then draw structural formulas for the following each. a PCI3 b CBr4 NH3 N2 e How many bonds can each of the following atoms form? Explain how you were able to determine the number a Nitrogern b. sulfur Oxygen d fluorine A halogen Carbon For naming molecular compounds apply the following rules: Name the first element in the molecular formula first using the element name without adding a suffix Name the 2nd element using the root of its name only and adding the suffix -ide . Use Greek prefixes (mono â 1, di â 2, tri â 3, tetra â 4, penta â 5. hexa â 6, octa,â 8, nona â 9, deca â 10) to indicate the number of atoms within that binary molecule. For Note: mono is not used as a prefix for the name of the first element. example, for CO2 we day carbon dioxide, not monocarbon dioxide 7. First, determine whether each of the following is an ionic or molecular compound. Then, apply the rules above, or the rules for ionic compounds, and name each of the following binary compounds: a P4010 bAl203 N203 d. SiF6

CHM 111 Lecture Notes - Lecture 17: Chemical Formula, Ionic Compound, Molar Mass

CHM 111 Full Course Notes

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