CHEM1006 Lecture Notes - Lecture 19: Sodium Fluoride, Chemical Formula, Structural Formula

55 views3 pages

skybee806

1 Aug 2016

School

Department

Course

Professor

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

Molecular formulas describe the exact number and type of atoms in a single molecule of a compound. The constituent elements are represented by their chemical symbols, and the number of atoms of each element present in each molecule is shown as a subscript following that element"s symbol. The molecular formula expresses information about the proportions of atoms that constitute a particular chemical compound, using a single line of chemical element symbols and numbers. Sometimes it also includes other symbols, such as parentheses, dashes, brackets, and plus and minus signs. For organic compounds, carbon and hydrogen are listed as the first elements in the molecular formula, and they are followed by the remaining elements in alphabetical order. For ionic compounds, the cation precedes the anion in the molecular formula. The molecular formula of sodium fluoride is naf. A molecular formula is not a chemical name, and it contains no words.

Related Questions

1. A 5.75 mL sample of mercury has a measured mass of 77.05 g. The density is ___________

2. Mercuryâs accepted density is 13.53 gÂ·mL^-1. The % error in your measurement is: ____________

Is this person accurate? ____ Is the person precise? ___

Defend your answer!

This molecule contains ____ elements and ____ atoms.

Carbon=black Oxygen=Red White=Hydrogen

The molecular formula for this substance is: ___________

5. Calculate the number of seconds in 5.25 years using unit analysis: (1 year = 365.25 days)

6. A calculator displays the answer to a problem as 53.29841

Report this answer to:

_______________ 5 significant figures

_______________ 3 significant figures

_______________ 1 significant figure

Which letter(s) represents: a) compound ____ b) pure element ____ c) Mixture of elements ____

d) Mixture of compounds _____ e) a solid element ____

skykoala735

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

1.Structural isomer refers to organic compound that have the same molecular formula but different structure (bonding pattern is different). This problem is designed to guide you to explore structure isomer.

(a)Go ahead and write Lewis structure for butane (C₄H₁₀). You may draw four C atoms connect straight as like in train.

(b)In the above structure, four C atoms are connected straight in a line. If you move one C atom to the side (like 3 C atoms in a line, one connected to the middle C atom), after you supply all the H atoms to make all the C atoms saturated with 4-bonds each. Will the molecular formula for your structure drawn be different from butane?

( c) Structures you obtained in (a) and (b) are an example of structural isomers. What kind of name we can give to structure in (b) so we can differentiate it from structure in (a)?

2.Alkane is the basic building block of organic compound. We often write alkane chain as a group R. On this basic chain, we can add different functional group, like âOH for alcohol, -COOH for carboxylic acid.

(a)Methanol refers to CH₃OH. Ethanol refers to CH₃CH₂OH. Draw the Lewis structure for these two compounds.

(b) If you have a straight alkane chain, where does âOH group can be attached? How do you name it so you can know where âOH group is attached?

3. Give the Lewis structure for CH₃COOH. Give its systematic name and common name.

4. Ester refers to two alkane chains connected through a single O atom. Write the Lewis structure for this simplest kind of ester: CH₃OCH₃. Find its name and some common use.

5. Benzene molecular formula is C₆H₆. The six carbon atoms are connected to form a ring (hexagon). Draw the Lewis structure for C₆H₆. Do you think the six bond lengths between C-C atoms should be same or not according to your drawn Lewis structure?

CHEM1006 Lecture Notes - Lecture 19: Sodium Fluoride, Chemical Formula, Structural Formula

Document Summary

Get access

Related textbook solutions

Chemistry: Structure and Properties

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related Documents

CHEM1006 Lecture Notes - Lecture 20: Isobutane, Chemical Formula, Butane

CHEM1006 Lecture Notes - Lecture 21: Sodium Fluoride, Valence Electron, Ionic Compound

CHEM1006 Lecture Notes - Lecture 22: Ionic Compound, Ionic Bonding, Oxidation State

Related Questions