(a)
Interpretation:
Whether the net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
(b)
Interpretation:
Whether the net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
(c)
Interpretation:
Whether the Net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
(d)
Interpretation:
Whether the Net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
(e)
Interpretation:
Whether the Net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
(f)
Interpretation:
Whether the Net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
(g)
Interpretation:
Whether the Net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
(h)
Interpretation:
Whether the Net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
(i)
Interpretation:
Whether the Net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
(j)
Interpretation:
Whether the Net charge for the
Concept Introduction :
Net charge of a molecule can be calculated by adding individual formal charges of each atom.
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure.
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Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
- ne has expired. The timer will c Your answers are saved automatically. Remaining Time: 44 minutes, 23 seconds. * Question Completion Status: A Moving to another question will save this response. Question 19 In which choice is the species correctly matched with its name? O NO3: nitrite ion O NO2 : nitrogen oxide O NO3: nitrogen trioxide ion O NO3 : nitrogen trioxide O All choices are correct. A Moving to another question will save this response. MacBook Pr 20 esc FT F2 F3 F4 F5 @ # 3arrow_forwardCan someone please show me how to figure these out? Thank you!arrow_forward27 Be sure to answer all parts. X 02:01:01 The following table gives numbers of electrons, protons, and neutrons in atoms or ions of a number of elements. Atom or Ion of Element Species A Species B Species C Number of Electrons 9 10 18 Number of Protons 9 19 Number of Neutrons 10 20 (a) Which of the species are neutral? A B C (b) Which are negatively charged? (c) Which are positively charged?arrow_forward
- Magnesium Salicylate is sold as an over - the - counter drug to treat pain and inflammation . If there are two salicylate ions for each Mg ion in the compound , what is the charge on the salicylate ion ? Explain your answer .arrow_forwardWhat is the relationship between the number of hydrogens in an acid and the charge on the anion that they are combined with?arrow_forwardAs seen in the table, compounds containing an integer ratio of elements depend on how many cations combine with how many anions to form a stable compound. For example, in table 1, to form a NaCl compound, first Na ionizes from the Na+ cation which is having +1 positive charge, which will lose 1 electron, it is having +1 charge, this electron then goes to Cl and it will change to Cl- anion by gaining the electron, so here 1:1 ratio charge which means 1 Na+ combines with 1 Cl-1 to form NaCl. So here integer ratio is 1:1 for this sodium chloride compound. As listed in table 2, Mg(OH)2, the integer ratio is 1:2 which means, Mg is a neutral atom that loses 2 electrons and forms an Mg+2 cation, which combines with OH which gains 1 electron to form OH- anion, So here Mg2+ can combine with 2 OH- anion, so they both combine to form Mg(OH)2 which has integer ratio as 1:2 . Thus, atom forms as ions by losing or gaining electrons and combines together in whole number ratio to form stable…arrow_forward
- Many common ionic compounds contain ions that are themselves composed of a group of covalently bonded atoms with an overall charge. True or false? Give some examples?arrow_forward1. Write formulas and names for compounds formed by the following positive and negative ions: a) Ba2+ and NO3- b) Al3+ and CO32- c) Pb2+ and CO32- 2. Write the cation and anion formulas (including charges) and the name of the following ionic compounds. (Use Roman numerals to indicate the charge on metals that can have more than one positive charge.) a) CaF2 b) TiO2 c) FeSO4 d) FeP e) NH4NO3 (this compound is composed of two polyatomic ions.) 3. Write formulas of the two ions in each compound and then write the formula of the compound. a) potassium iodide cation: K+ inputted as K^+ anion: I- inputted I^- formula: KI b) aluminum hydroxide c) sodium phosphate d) sodium phosphide e) copper(II) sulfidearrow_forwardPlease help me solve the following question and please please make sure everything is correct ! its important thanks !1arrow_forward
- 1) Provide an explanation for the way the following formula Ca5(PO4)3OH is written and provide the name of all the ions involved. (what do the subscripted numbers indicate, why is PO4 in brackets) 2)Thinking of the individual charges of the metal and polyatomic ions present in Ca5(PO4)3OH, can you explain why this compound is neutral? Show the working of how the charges balance each other out. Q3. A compound has the general formula X2O, with X representing an unknown element or Ion and O representing oxygen. Which of the following could NOT be a name for this compound? Explain your answer. a. sodium oxideb. iron(II)oxide c. copper(I)oxided. dinitrogen monoxidee. water Q4. Consider a hypothetical simple ion M2+. Determine the formula of the compound this ion would form with each of the following anions. a. hydroxide b. nitrite Q5. A metal ion with 2+ charge has 23 electrons and forms a compound with a halogen ion that contains 17 protons. a. what is the identity of the metalb. what is…arrow_forward2. 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.arrow_forwardplease answer these question correctly: 1. For a group 13/3A atom, how many electrons must it lose to be stable? 2. For a group 13/3A atom, how many electrons must it gain to be stable?arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning