CHEM 151 Lecture Notes - Lecture 3: Ketone, Viscosity, Metalloid

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ultramarinehornet287

20 Aug 2016

School

University of Arizona

Department

Chemistry

Course

CHEM 151

Professor

Bobbi Anglin

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Document Summary

Molecular vs ionic compounds: molecular all of the atoms that make up a chemical substance belong to nonmetal elements, ionic atoms that make up a chemical bond are metallic and nonmetallic. Molecular compounds: covalent bonds bond between two nonmetals. They are highly directional because the chance of finding bonding electrons outside the region between the two bonded atoms is low. They emerge from the dynamic interactions between the many molecules that form a substance. Intermolecular forces or imfs: these are dependent on the proximity of the molecules, the amount of protons and electrons and the attractive and repulsive forces between protons and electrons. Polarizeability the extent to which charge distribution in the atoms that make up a substance is affected by the presence of external charge. Dependent on the number of electrons and the space they occupy. Meaning that fluorine is not very polarizeable because it keeps its electrons close. Bond polarity the difference in charges of a bond.

Related Questions

13%â¡ 8:08 PM ì docs.google.com Covalent Bonding and lonic Bonding study guide T-Mobile LTE Noteâ compare and contrast does not mean state one similarity and one difference Go back to our thinking maps and metacognitive logs and review everything we learned. Differentiate between the following: Atom, element, compound, bond, electron. Click here for a short video 2 Compare and contrast ionic and covalent bonds including the nature of the bonds. Click here for a video comparing the 2. Click here for a video on covalent bonding. s Explain the rules used for naming ionic compounds as well as those used for naming molecular compounds. You can either create 2 lists or 1 double bubble. 4 Use the periodic table to indicate whether the following molecules are ionic or covalent. Work each problem using either the diagram for transfer or sharing, then write the chemical formula and finally name each compound correctly. a NaBr b. HF d H20 s Explain why all of the following compounds will be molecular, then draw structural formulas for the following each. a PCI3 b CBr4 NH3 N2 e How many bonds can each of the following atoms form? Explain how you were able to determine the number a Nitrogern b. sulfur Oxygen d fluorine A halogen Carbon For naming molecular compounds apply the following rules: Name the first element in the molecular formula first using the element name without adding a suffix Name the 2nd element using the root of its name only and adding the suffix -ide . Use Greek prefixes (mono â 1, di â 2, tri â 3, tetra â 4, penta â 5. hexa â 6, octa,â 8, nona â 9, deca â 10) to indicate the number of atoms within that binary molecule. For Note: mono is not used as a prefix for the name of the first element. example, for CO2 we day carbon dioxide, not monocarbon dioxide 7. First, determine whether each of the following is an ionic or molecular compound. Then, apply the rules above, or the rules for ionic compounds, and name each of the following binary compounds: a P4010 bAl203 N203 d. SiF6

Chemistry 162 Lab Activity

Introduction Water has an amazing ability to adhere (stick) toitself and to other substances. Hydrogen bonds form when hydrogenatoms covalently bonded to nitrogen (N), oxygen (O), or fluorine(F) in the form of covalent compounds such as ammonia (NH3), water(H2O) and hydrogen fluoride gas (HF). In these molecules, thehydrogen atoms do not pull as strongly on the shared electrons asthe N, O, or F atoms. Therefore, the molecules are polar; thehydrogen atoms become positively charged and are able to formhydrogen bonds to negative ions or negatively charged parts ofother molecules (such as the N, O, and F atoms that becomenegatively charged in these compounds). Hydrogen bonds are not truebonds like covalent bonds or ionic bonds. Hydrogen bonds areattractions of electrostatic force caused by the difference incharge between slightly positive hydrogen ions and other, slightlynegative ions. These attractions are much weaker than true ionic orcovalent bonds, but they are strong enough to result in someinteresting properties.

In the case of water, hydrogen bonds form between neighboringhydrogen and oxygen atoms of adjacent water molecules. Theattraction between individual water molecules creates a bond knownas a hydrogen bond (Fig. 1).
Fig. 1: Hydrogen bonds shown as the dotted lines between watermolecules.
Cohesion Molecules of pure substances are attracted to themselves.This sticking together of like substances is called cohesion.Depending on how attracted molecules of the same substance are toone another, the substance will be more or less cohesive. Hydrogenbonds cause water to be exceptionally attracted to each other.Therefore, water is very cohesive.
Adhesion Adhesion is similar to cohesion, but it involves unlike(i.e. different) substances sticking together. Water is veryadhesive; it sticks well to a variety of different substances.Water sticks to other things for the same reason it sticks toitself â because it is polar so it is attracted to substances thathave charges. In this lab activity, you will be asked to use thematerials and procedures provided to explore the properties ofwater that involve both cohesion and adhesion. Be sure to writedown your observations and results as you progress. sults as youprogress.

Fig. 1

Hydrogen bonds shown as the dotted

lines between water molecules.

Part 1:

Exploring Water

Procedure

How many drops of water can you fit on the surface of a pennywithout the water spilling over?

Predict how many drops of water will fit on a penny. Record yourprediction.

Use the plastic pipette to drop water on the surface of a penny.Drop car

efully and slowly to fit as

many drops as possible on the penny. Count each drop until thewater spills over the side of the

penny and record your results.

Compare your results to those of your classmates. Record therange and calculate the average

number

of drops that fit on a penny.

Add more drops to the penny, without letting the water spillover. Carefully observe and draw the

water on the penny.

Record

a hypothesis for the behavior of water that you observed, usingthe language of cohesion

and adhesion

in relation to the water and the penny.

Record your results and

thinking in your notebook.

Can you

disturb

the water on the penny without spilling it?

dd drops of water to the penny, until the water is almost readyto spill over.

Predict what will

happen when you insert a toothpick into the surface of the waterpiled on the

penny. Record your prediction.

Insert the

toothpick

and carefully observe the surface of the water.

Try inserting the

toothpick

in various ways. Observe the surface of the water.

Pay special attention to

the water surface where the skewer enters the water.

Record your observations and draw what you see.

Repeat

these

procedures using a paper clip and the metal clip part of abinder clip. Try to indent the

pile of water as much as p

ossible without spilling it.

Record your observations and dra

w what you see, paying careful

attention to the surface of the

water.

Record

a hypothesis for the behavior of water that you observed usingthe language of cohesion

and adhesion in relation to the

toothpick

, the paperclip, the binder clip, and the water.

Record your results and

thinking in your notebook.would you please answer the questionfor me . Thanks

CHEM 151 Lecture Notes - Lecture 3: Ketone, Viscosity, Metalloid

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