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Ch. 2 - Water and Carbon: The Chemical Basis of Life
Freeman - Biological Science 8th Edition
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Tutti i libri di testoFreeman 8th EditionCh. 2 - Water and Carbon: The Chemical Basis of LifeProblema 6
Capitolo 2, Problema 6

Locate fluorine (F) on the partial periodic table provided in Figure 2.2. Predict its relative electronegativity compared to hydrogen, sodium, and oxygen. State the number and type of bond(s) you expect it would form if it reacted with sodium (Na).
Partial periodic table showing elements including fluorine, sodium, and hydrogen for chemistry study.

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1
Locate fluorine (F) on the partial periodic table. It is in group 17 and period 2.
Understand that electronegativity increases across a period from left to right and decreases down a group.
Compare the positions of hydrogen (H), sodium (Na), and oxygen (O) relative to fluorine (F) on the periodic table.
Predict that fluorine (F) has higher electronegativity than hydrogen (H), sodium (Na), and oxygen (O) because it is further to the right and higher up on the periodic table.
Determine that fluorine (F) would form an ionic bond with sodium (Na) by gaining one electron from sodium, resulting in a Na+ cation and an F- anion.

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Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons when forming chemical bonds. It is a key factor in determining how atoms interact with each other. In the periodic table, electronegativity generally increases from left to right across a period and decreases from top to bottom within a group. Fluorine, being in the top right corner, is the most electronegative element, which means it has a strong tendency to attract electrons compared to hydrogen, sodium, and oxygen.
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Covalent Bonds

Ionic Bonding

Ionic bonding occurs when one atom donates an electron to another, resulting in the formation of charged ions. This type of bond typically forms between metals and nonmetals, where the metal loses electrons and the nonmetal gains them. In the case of sodium (Na) and fluorine (F), sodium will lose one electron to become Na+, while fluorine will gain that electron to become F-. This transfer of electrons leads to the formation of an ionic bond between the two elements.
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Ionic Bonds

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. These trends include variations in atomic size, ionization energy, and electronegativity. Understanding these trends helps predict how different elements will interact chemically. For example, as you move from sodium to fluorine, the increasing electronegativity of fluorine indicates it will form a stronger bond with sodium than sodium would with hydrogen or oxygen.
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Variables
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Consider the reaction between carbon dioxide and water to form carbonic acid: CO2(g)+H2O(l)⇌CH2O3(aq) In the ocean, carbonic acid immediately dissociates to form a proton and bicarbonate ion, as follows: CH2O3(aq)+H+(aq)⇌CHO3−(aq) If an underwater volcano bubbled additional CO2 into the ocean, would this sequence of reactions be driven to the left or the right? How would this affect the pH of the ocean?

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What factors determine whether a chemical reaction is spontaneous or not?

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Which of these functional groups is known to be used for storing large amounts of chemical energy?

a. Amino group

b. Carbonyl group

c. Phosphate group

d. Sulfhydryl group

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When H2 and CO2 react, acetic acid can be formed spontaneously while the production of formaldehyde requires an input of energy. Which of these conclusions can be drawn from this observation?

a. More heat is released when formaldehyde is produced compared to the production of acetic acid.

b. Compared to the reactants that it is formed from, formaldehyde has more potential energy than does acetic acid.

c. Entropy decreases when acetic acid is produced and increases when formaldehyde is produced.

d. Only acetic acid could be produced under conditions that existed in early Earth.

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Which of these molecules would you predict to have the largest number of polar covalent bonds based on their molecular formulas?

a. C2H6O(ethanol)

b. C2H6(ethane)

c. C2H4O2(acetic acid)

d. C3H8O (propanol)

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