Chemistry Chapter 10 Review Answers

Answers to Chapter 10 Study Questions

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15286

ane.

1. NH _iii (H-bonds)/PH _iii (dipole); NH ₃
2. both LDF; C ₆ H ₁₄ (higher molar mass)
3. CO ₂ (LDF)/H ₂ O (H-bonds; H_twoO) (also, H ₂ O is a liquid, while CO _ii is a gas)
4. HCl (dipole)/LiCl (ionic); LiCl
5. Na (metal)/NaCl (ionic); NaCl

2.

1. Ionic solids are equanimous of positive and negative ions bundled so that each positive ion is surrounded past negative ions and vice versa. The are held together past the attractive force betwixt the oppositely charged ions. Some examples are NaCl, NaNO ₃ , MgSO ₄ , CuCl ₂ .
2. Covalent (molecular) solids are made upward of molecules. Covalent bonds hold together the atoms within the molecules. The forces between the molecules are dispersion and dipole forces and hydrogen bonds. Examples include water (H _two O), ammonia (NH ₃ ), table sugar (C ₁₂ H ₂₂ O ₁₁ ), CO ₂ .
3. Metallic solids are made up of a regular crystalline array of metal atoms. Valence electrons are gratis to move within the solid and make upward the "metallic bonding" that holds the metallic together. Some metallic solids are aluminum, gilt, iron, nickel, copper, zinc, sodium.
4. Network covalent solids consist of atoms covalently bound together in a continuous three-dimensional network. The solid is held together by covalent bonds. Examples are diamond (C), carborundum (SiC) and quartz (SiO ₂ ).

3. In general, b) molecular < c) metallic < a) ionic < d) covalent network

4. Merely metallic substances conduct electricity as solids. Both metallic and ionic substances conduct electricity as liquids.

v.

1. F_two (molecular, LDF)
2. NaCl

six. The boiling point of a liquid is the temperature at which its equilibrium vapor pressure is equal to external pressure. The disquisitional temperature is the highest temperature a substance tin can exist liquified; higher up the critical temperature a substance is a gas at whatever pressure. The critical pressure is the pressure needed to liquify a substance at its critical temperature. The triple point is the temperature and force per unit area at which solid, liquid and gas all exist in equilibrium.

seven.

1. no alter
2. vapor pressure level increases with increasing temperature
3. higher intermolecular forces mean lower vapor pressure level
4. no modify

viii. London dispersion forces (van der Waals forces) < dipole-dipole forces < hydrogen bonds.

9.

2. O _two (s) is denser than O _ii (fifty) because the solid-liquid line on the phase diagram is normal (slants slightly to the right).
3. O _ii will melt when heated at a pressure level of 1 atm.

10. Showtime find the number of moles of iodine in the flask, using the ideal gas police:

P = 0.466 mmHg = 6.13 x x ^-four atm; T = 30°C = 303 K; V = 1.00 50; north = ?

\(\mathrm{n=\dfrac{PV}{RT}=\dfrac{(6.13\times10^{-4}\:atm)(1.00\:Fifty)}{(0.0821)(303\:K)}=2.46 \times 10^{-5}\: moles}\)

\(\mathrm{two.46\times10^{-v}\:moles\times\dfrac{253.eight\:g\:I_2}{1\:mole\:I_2}\times\dfrac{1000\:mg}{1\:m}=6.25\:mg}\)

Chemistry Chapter 10 Review Answers,

Source: https://chem.libretexts.org/Bookshelves/General_Chemistry/Exercises%3A_General_Chemistry/Exercises%3A_Zumdahl_and_Zumdahl/Homework_Solutions/Answers_to_Chapter_10_Study_Questions

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