Topic 2: ChemistrySection 2.1Elements -Atom -Figure 2.1 – What does the periodic table show?Subatomic particles: see Figure 2.3ParticleMass (a.m.u.)ChargeLocationIsotope –Section 2.2What is the major topic of this section?What three types of bonds are discussed in this section? (See table 2.1)What is the difference between a covalent bond and an ionic bond? (See Figures 2.5 and 2.6)Describe the shape of a water molecule and explain why the molecule is "polar". (Figure 2.7)Hydrogen bond –pg. 3 What are the four most common elements in living organisms? (Table 2.2)Read the chapter summary for sections 2.1 and 2.2 on page 44.Read the Concept Review:1-5 on page 45.Test Yourself:1.2.3.4.15.Section 2.3What is the topic for this section?Why does life depend on water?What is the difference between a solute and solvent?Hydrophobic –Hydrophilic –Why do ions dissolve in water? (Figure 2.8)Figure 2.9 – Why do you think ice floats? Why do you think this is important to life on earth?Section 2.4What is the difference between an acid and a base?What is the pH scale? (See Figure 2.10)pg. 4

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Section 2.1 Elements - Atom - Figure 2.1 – What does the periodic table show? Subatomic particles: see Figure 2.3 Particle Mass (a.m.u.) Charge Location sotope – Section 2.2 What is the major topic of this section? What three types of bonds are discussed in this section? (See table 2.1) What is the difference between a covalent bond and an ionic bond? (See Figures 2.5 and 2.6) Describe the shape of a water molecule and explain why the molecule is "polar". (Figure 2.7) Hydrogen bond - pg. 3

Section 2.1 Elements - Atom - Figure 2.1 – What does the periodic table show? Subatomic particles: see Figure 2.3 Particle Mass (a.m.u.) Charge Location sotope – Section 2.2 What is the major topic of this section? What three types of bonds are discussed in this section? (See table 2.1) What is the difference between a covalent bond and an ionic bond? (See Figures 2.5 and 2.6) Describe the shape of a water molecule and explain why the molecule is "polar". (Figure 2.7) Hydrogen bond - pg. 3

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter13: The Geometrical Structure Of Molecules-an Experiment Using Molecular Models

Section: Chapter Questions

Problem 2ASA: The model consists of balls and sticks. a. How many holes should be in the ball you select for the N...

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The model consists of balls and sticks. a. How many holes should be in the ball you select for the N atom? ___________ b. How many holes should be in the ball you select for the H atoms? ____________ c. How many holes should be in the ball you select for the Cl atom? ____________ The electrons in the molecule are paired, and each stick represents a valence electron pair. d. How many sticks do you need? ____________
5. Which of the following statements is incorrect? A. AICI3, Ba(NO3)2, and CuSO4 are examples of ionic compounds. lonic solids dissolved in water dissociate to form ions В. C. lonic bonds are formed between metals and nonmetals. D. When forming ionic bonds, metals and nonmetals share electrons.
What is an atom?What is atomism?What is alchemy?What is protoscience and pseudoscience?What is atomic theory?On a bond paper, draw the different model of an atom.
1.) An element X reacts with hydrogen to form a compound of formula HX. In which group in the periodic table is X most likely to be found? a. 1A b. 2A c. 7A d. 8A 2.) Which of the following compounds has the strongest chemical bond? a. salt b. sugar c. water d. ethanol
What are allotropes? Give an example. How are allotropesdifferent from isotopes?
5. Fill in the empty boxes with the correct information. 6. 1st Element Ag # of atoms 1 b. Ionic bond: 2nd Element c. Polyatomic Ion NO₂ # of atoms Give three chemical formulas and corresponding names for each bonding pattern: a. Covalent bond: 81 Formula C8H10 Name Ammonium phosphate Molybdenum (II) acetate Potassium tellurate
9. Which pair of atoms would form an ionic bond? a. bromine and oxygen b. chlorine and lithium c. carbon and nitrogen d. sodium and neon e. copper and chromium 15. Using only the periodic table, place the following atoms in order of increasing atomic radius: C, Ba, 0, Ca, and Ge. 21. What types of elements are bonded together to make an ionic compound? Give three examples of ionic compounds. Identify the types of elements that make up the compound in each example. 27. Describe how the physical state of a substance at room temperature depends on the strength of the intermolecular forces between the particles of the substance.
3. During the formation of ionic bonds, with which noble gas does boron become isoelectronic with? 4. What is a diatomic molecule? Give an example of a diatomic element and draw its Lewis dot diagram.
2. Look at the Periodic Table and answer these questions. a. Do nonmetals form anions or cations? b. Do metals form anions or cations? c. What is the charge for all of the elements in Group 1? d. What is the charge for all of the elements in Group 2? е. What is the charge for all of the elements in Group 17? f. Do cations bond with other cations? g. Do anions bond with other anions?
2. Draw the Lewis dot structure for CH;NO, in which the atoms are arranged C-O- N-O, and the hydrogen atoms are attached to the carbon atom.
Q4. Thinking of the individual charges of the two polyatomic ions present in (NH4)2CO3, can you explain why this compound is neutral in charge? Show the working of how the charges balance each other out.
Part 1: Nomenclature What are covalent compounds (molecules)? Give two examples of covalent compounds and their formula. What are binary ionic compounds (formula units)? Give two examples of binary ionic compounds and their formula What is the difference between naming of cations with variable charge and compounds with fixed charge? Give two examples of each and their formula What are polyatomic ions? Give two examples of polyatomic ions and their formula Give two examples of compounds containing polyatomic ions and their formula Give an example of names of binary acids (not containing a polyatomic ion) in aqueous solution and its formula. Give an example of an oxyacid (containing a polyatomic ion) inn aqueous solution and its formula. Part 2: Structure, Shape and polarity Draw the Lewis structure of PH3 draw the electronic geometry and name the geometry (hint: very similar to NH3) draw the molecular geometry and name the…