much larger than the density of steam. Notice that the densities and molar volumes of ice and liquid water are much closer to each other than to steam ...... vaporize 90.0 g of C3H7OH at its boiling point. 78 because the given amount of C. 3. H. 7. O
Ionic Bonding and the Crystal Lattice. â¢ The extra ... are polar with a higher density of bonding electrons ... both bonds as well as the non-bonding valence shell ...
If you can DO them, check the box If you CANNOT do them, write some notes. TO YOURSELF about what you need to ... M b. in a crystal ofthe salt NaCl Em _ 549A 0 in a solution of potassium nitrate KNO3 i mm! id bib A d'. in diamond ... poor conductor o
Vapor Pressures of Various Liquids. Temperature. (°C). Ethyl. Alcohol. (mmHg) ... Ex1. A beaker of benzene (C6H6) is at room temperature (20° C). What is its ...
You may graph these on the graph paper box or use the online tools or use a larger piece of graph paper. Trend in Halogens. 1. Graph the molar enthalpy of ...
... the following substances form in its solid state? Choices to consider are metallic, ionic, covalent, or molecular crystals. (a) C2H6 ______. (b) Na2O ______ (c) ...
reduce the cost of textbook materials for the K-12 market both in the U.S. and ... in the formation of a nonpolar covalent, polar covalent, or ionic bond. 1.
6. Identify the type of IMF for each molecule. Molecule. Strongest IMF. H2O. H2S. H2Se. H2Te. 7. Explain the general shape of this graph. 8. Account for the trend ...
... interaction involves the attraction between a fully charged entity and a polar molecule. .... Commons). http://commons.wikimedia.org/wiki/File:Dipole-di.
pioneer the generation and distribution of high-quality educational content that will ... a chemical bond is predictive of the type of bond made by those two atoms.
terms âFlexBookÂ®â and âFlexBook PlatformÂ®â (collectively. âCK-12 Marksâ) ... The two chlorine atoms share the pair of electrons in the single covalent bond equally, and the electron density surrounding ... A polar covalent bond is a cov
Step 1: List the known quantities and plan the problem. Known ..... Ethanol and dimethyl ether both have the same molecular formula, C2H6O. However, the ...
3. With which type of substances do London dispersion forces play the most significant role? a) polar molecules d) non-polar molecules b) metals e) network compounds c) ionic compounds. 4. The heat of vaporization of H2S, at its boiling point. (â61
South Pasadena â¢ AP Chemistry. Name. Period ___ Date ___/___/___. 13 â¢ IMF's, Liquids, & Solids. I M F ' S I N S O L I D S. Indicate the strongest IMF holding together crystals of the following: Molecular Crystal. Metal. Ionic Crystal. Network So
This diagram shows what happens to particles during changes of state. This is ... moving faster and faster. More and more heat absorbed rni.lfWI. Solid. Liquid.
mixture may retain their individual properties when combined, or the ... properties, sand, shape, size, solid, solution, states of matter, substance, surface,.
All states of matter have a fixed mass and fixed volume. _____ 7. The volume and shape of a solid can never change. _____ 8. Surface tension explains why ...
be for the noble gases and non-polar molecules such as helium, neon, argon, krypton, xenon, hydrogen, oxygen, methane, carbon dioxide, and so forth.
a type of strong polar attraction between a hydrogen atom in one molecule and .... A homologous series of compounds are compounds where the elements of a ...
Hydrogen bonding: 3. London dispersion forces: B. For each of the following compounds, draw the Lewis structures, indicate the type of bonds in each, draw any ...
bonds in the liquid state: ... (g) NH3. CH4. (h) HCl(g). NaCl. (i) SiC. Cu. 3. Isopropyl alcohol has a melting point ... a) Which substance can form hydrogen bonds?
Methanol, CHgOH, (molar mass 32.04 g/mol) has a heat of vaporization of 39.2 kJ/mol and a density of. 0.7914 gij. New much energy is needed to vaporize 350. mL of r'netbanol'IJ to). 350. ML CHyDHV :1qu 5' w 7 MS: 3 a}; Rs lee he 32,0110 1. 3. The gre
These three states of matter are common on Earth. ... are found in fluorescent lights, plasma TV screens, and plasma balls like the one that opened this chapter.
13Intermolecular Forces, Liquids, and Solids The four types of solids
Intermolecular Forces of Attraction • Ch 12 was all about gases… particles that don’t attract each other.
Intermolecular Forces of Attraction • Ch 13 is about liquids and solids… where the attraction between particles allows the formation of solids and liquids.
Intermolecular Forces of Attraction • These attractions are called “intermolcular forces of attractions” or IMF’s for short.
Covalent Network Solids • Crystal held together with covalent bonds
Covalent Network Solid Examples • • • • • • •
C(diamond) C(graphite) SiO2 (quartz, sand, glass) SiC Si WC BN
Properties of Metals Metals are good conductors of heat and electricity. They are shiny and lustrous. Metals can be pounded into thin sheets (malleable) and drawn into wires (ductile). Metals do not hold onto their valence electrons very well. They have low electronegativity.
Properties of Ionic Solids • • • •
Brittle High MP & BP Dissolves in H2O Conducts as (l), (aq), (g)
Intermolecular Forces (IMFs) • Each intermolecular force involves + and – attractions. • The list from weakest to strongest is: – London Dispersion Forces – Dipole-dipole interactions – Hydrogen bonding – Ion-Ion Interactions
Ion-Ion Interaction • + ion attracts a – ion (opposites attract) • Lattice energy is a measure of the strength of this interaction • NaCl(s) + energy Na+(g) + Cl-(g)
Dipole-Dipole Interaction • Same idea as ion-ion interaction, but not as strong because the charges are only “partial charges”. • Polar molecules have this kind of IMF.
Hydrogen Bonding • This is a special case of dipole-dipole interaction (about 10x stronger). • H-O, H-F, H-N – Atoms are small and electronegative – Very polar bond leads to stronger IMF
London Dispersion Forces
London Dispersion Forces • Every atom attracts every other atom with this force. (H-bonding & LDF, Dipole & LDF) • +/- attraction again but the polarity is only temporary. • LDF is stronger with a “more polarizable electron cloud”. (use these words in FRQ) – More electrons – Larger atoms or longer molecules
Examples to Recognize • London dispersion forces – non-polar molecules and other molecules, too. • Dipole-dipole interactions – polar molecules. • Hydrogen bonding – polar molecules with – H-O (water, alcohols, oxoacids) – H-N (ammonia, amines) – H-F (HF)