8: Solids, Liquids, and Gases
- Page ID
- 15927
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Most of us are familiar with the three phases of matter: solid, liquid, and gas. Indeed, we addressed the energy changes involved in phase changes. The substance we are probably most familiar with has those three phases: water. In everyday life, we commonly come in contact with water as a solid (ice), as a liquid, and as a gas (steam). All we have to do is change the conditions of the substance—typically temperature—and we can change the phase from solid to liquid to gas and back again. Under the proper conditions of temperature and pressure, many substances—not only water—can experience the three different phases. An understanding of the phases of matter is important for our understanding of all matter. In this chapter, we will explore the three phases of matter.
- 8.0: Prelude to Solids, Liquids, and Gases
- This page explains that carbon dioxide turns into solid dry ice at around -78°C, skipping the liquid phase. It highlights the risks of dry ice, including tissue freezing and oxygen displacement, requiring safety precautions. The page also notes its various applications in refrigeration, preserving medical items, dermatological treatments, and cooling transplant organs for surgery.
- 8.1: Intermolecular Interactions
- This page explores phases of matter (solid, liquid, gas) and their dependence on temperature and pressure, highlighting the influence of intermolecular forces on melting and boiling points. It discusses polar and nonpolar molecules, with hydrogen bonding as a significant factor in boiling points, especially in substances like water. The page also details DNA's double-helix structure, emphasizing hydrogen bonds' role in replication.
- 8.2: Solids and Liquids
- This page discusses the differences between solids and liquids, both categorized as condensed phases due to close particle proximity. Solids maintain fixed positions, definite shapes, and volumes, while liquids allow for particle movement with a definite volume but no fixed shape. It highlights water's unique properties, including high melting/boiling points, density variations, and significant heat capacity, underlining its vital role in supporting life on Earth.
- 8.3: Gases and Pressure
- This page explains the gas phase as a unique state of matter characterized by the kinetic theory of gases, which posits that gases are made of rapidly moving particles with significant separation that lack attractions. The theory, influenced by scientists like Robert Boyle, describes key properties, including the relationship between pressure and particle collisions, with units of measurement such as pascals, bars, atmospheres, and torr.
- 8.4: Gas Laws
- This page covers various gas laws, including Boyle's Law and Charles's Law, which describe the relationships between pressure, volume, and temperature of gases. It explains the ideal gas law for predicting gas behavior, Dalton's Law of Partial Pressures for gas mixtures, and Henry's Law for gas solubility in liquids.
- 8.E: Solids, Liquids, and Gases (Exercises)
- This page explores intermolecular interactions like ionic and hydrogen bonding, and compares covalent network and molecular compounds. It discusses the properties of solids, liquids, and gases, alongside the concept of pressure in gases using kinetic theory and gas laws. The page includes practical exercises for calculating gas behavior, addressing volume, temperature, and pressure changes and their implications in reactions and phase changes, with real-world applications like tire inflation.
- 8.S: Solids, Liquids, and Gases (Summary)
- This page explores the phases of matter—solid, liquid, and gas—highlighting the influence of intermolecular interactions on their characteristics. Strong interactions define solids, while weaker ones in liquids and gases enable flow and expansion. Key concepts covered include hydrogen bonding, polar/nonpolar interactions, dispersion forces, and the kinetic theory of gases.
Thumbnail: A water drop. (CC BY 2.0; José Manuel Suárez via Wikipedia).