Name: Unit 1: States of Matter and Intermolecular Forces
Brand: EduBirdie
Rating: 5.0 (13 reviews)

University:
High School
Course:
High School Chemistry
Academic year:

2019
Views:

365

Pages:

6
Author:

46280dk

UNIT 1: STATES OF МАТГЕR & INTERМOLECUI.AR FORCES: Ho\t Chernistry: & GAS 1.А WS: Holt Chernistry: UNIT GOALS: the student will Ье аЫе to describe how intermolecular forces affect properties such as states of rnatter and boiling point; the student will Ье аЫе to describe the uniqueness of the gas state and its' relationships with ternperature, pressure, and volurne OB.JECГIVES; Тhе learner wil\ ... 1. reiate the properties of а state to the energy content and particle arrangernent of that state of matter 2. identify all changes of state 3. explain energy changes and entropy changes during changes of state , 4. contrast ionic and rnolecular substances in terms of their physical characteristics and types of forces " 5. describe intermolecular forces between polar molecules 6. describe hydrogen bonding 7. describe intermolecular forces between non-polar rno\ecules 8. re\ate types of forces to strength and relative boiling points 9. understand the role of vapor pressure in changes of state between а liquid and а gas 10. Ье аЫе to read а vapor pressure graph to deterrnine boiling point at various pressures 11. describe the general properties of gases 12. define pressure and convert between various units of pressure 13. relate kinetic-molecular theory to properties of gases 14. state Boyle's law and use it to solve proЬlems involving pressure and volume 15. state Charles' law and use it to so\ve proЫems involving ternperature and vol·.•me 16. Ье аЫе to use the comЬined gas law to solve proЬ!ems involving pressure, temperature, and volume 17. state Avogadro's \aw and solve proЫems involving molar volume 18. explain the relationship between diffusion and gas particle size UNITTEST: Date·due -------TEST REVIEW: (due before the test) 1. Draw particle diagrams to represent the 3 states of matter for а single element: Solid Liquid Gas о о о о о С) -о Ь· о ; \ � q.._ JL s:j.- J0 м е- t +- q..._ GrJpV J . c.,oV'-J..eлs-e � � . fге.е. -=с- -е__ � S а. Which ones are increasing in entropy? Give а reason for your answer. 17 i;:.C.. \.t ·, �-rR D Р�·о \..:) (\ � V � Lo EN -ГR.а ?-у • t;.tJ"f" 3. Describe the difference bet{;een evaporation and boiling? ➔. . . . р . Q.r р L [v'AP-":1 · • ➔ " 1oiJt._, (_м/t-1М) '? S,usJ:"0<. i:__� ().._"'" br\ly +-e..""'-r L\ \JD-'?t>C Pr е,,5:, �it:,:i:мr;;- L� (д 70 60 :r: 50 Е f ::, gJ о .> - -~- �. о � / j/ . -L---v ' � (К� s_) .� L.o с I мР / / А/ t--, Ро lcv- � - 1 1; 300 100 / 1/ / 400 �0 1\__ в. 1 о 200 �, VV\ о r е.. ('_,�е Pre-s -.1-- A:+v'\.. 4 � ь ') 800 5$ ..,, д-+м. .::, \Л Ь. What type of subs\ances have higher boiling points? Ве sure to use forces 10 your answer. The graph below shows the vapor pressure curves for liquidsA and Ч� liY"I.. Q(\} а. What value must Ье known in order to state the boiling oint of а liquid? М. о -r с \_р,_, 1� Questions through t refer to the following: f бсi . v v , / / . О 10 20 30 40 50 60 70 80 90 100110120 Temperature ("С) According to the diagram, \vhat is the vapor pressure of Iiquid at ° А 70 С? [Уоиr answe1· must iпclude сттесt units.] (о� о VV'-""- \.\� According to �he diagram, at what ternperature docs liquid В have the ·same vapor pressure as liquid А at 70 ° С? [Уоиг _ answer must mcl11de сттесt zmits.] \\� оС, Wt1ich liquid in thc given diagram will evaporatc тоге rapicily? [Explai n уоиг апsи·ег in tenns oj" iтеmю!еси/аг Jiнce�? �� Н--1tи • \) r � :::; \!J,Q_°'-'k�v \ t1 F E:,\J АР �s � As thc tempcrature of а liquid ihcreases, its А) rcmains thc samc � prcssurc � � incrcascs С) dccrcascs According to Vарог Ргеssиге of Four Liquids chcmistry refercnce tаЫс, what is thc vapor pressurt of propanonc at 45 °С? С) 33 kPa @:)10. kPa А) 98 kPa D) 22 kPa According to the Vарог P,·essuгe of Fош· Liquids chemistry reference tаЬ!е, what is thc boi]ing point,of ethanoic acid at 80 kPa? В) 125 ° С @)111 ° с 10. С) 100 ° С D) 28 ° С Using your knowledge of chemistry апсt· the information in the Vapo1· Ргеssш·е ofFоиг Liquids chemistry reference tаЫе, wblch statement concerning propanone and water at 50 ° С is true? ф А) Propanone has а lowervapor pressure and weaker intermolecular forces than water. Propanone has а higher vapor pressure and stronger intermolecuiar forces than water. Propanone has а higher vapor pressure and weaker intermolecular forces than water. ) Propanone has а lower vapor pressure and stronger intermolecular forces than water. Arrange the following in order of highest ВР to lowest ВР: а. polar molecules, ionic compounds, non-polar molecules ';t:ON\L :, r'<:>t�, 1 fs:Jt" Р ( LJ�/"-� - !!> L� &r') C..L ;\.. ') O d-- ) �-а-) \-\--; ь. N2, с12, 02, н2 - aJ l N с. НС!, NaBr, Н20, СН4 ��\)� _., 1-1 °d-O t..L ., 1 r: • 1> -:Со,-, с:. �\а., �\С:, е:ь '?.,Нk1., ,..,�О'-. i;;:.. d. КF, HF, F2, PF3 t<-P _,, l-t F' - PF], � y°d::Co,-\,L Po\��•%:e:t, �.Р Pc, lc,,_, How is hydrogen bonding different than the intermolecular force between other polarmolecules?yo\ l� 'J olra� М-o\E>__�LL\e__s Cl, С..�ч ....sl"' w\ а. What are the two conditions for a(\s�bstance to have hydrogen bonding? � у'о \ с,._г М...t) \е_ �u-..)LJ( ! \-\ 'j сlго c,...vv\. -F _ Ь. Identify 3 substances With hyd№gen-bonding: \� -\-\-\ r > 1-1 &о, ) � \-\� ___,, _,,, w What does SТР stand for? 1Where can you find these values on your Reference (л'\ А ТаЫеs? ,S...�г� �М.х> ). -e__s 51Л ,r-е._ . €_. \.J:iJ а. List the values from this tаЫе. -та:_ 1о l ?г 1 � Jl3'\( ) 0 ° � \Vhy must you state temperature and pressure when discussing gas volume? �� \J��CL_ �� ·w � Molecule 1. NНз -'½'½;':) � <:)� '< 2. 02 !t � ;,..оt--1 � \-\ 1-\ '01�\ t 4. Ar ',('"'о�: о: /j , <:ь .,, \ S,д_) l�] �l� Цг 5. Н2О "-"' 1-\ "-" о';;; , tt 1-\- '),1-. 6. СН4 0 с::_ � '< ,,,.\\s);:;,, 7. MgO 8. РСlз -tlr !� \ С:,, s�, о .!J \/:'\ (i' '1' .,_) -:'-} \ E, ,J�o 9о\ог �'i чУ\ �()+6У,"{ vo\цr �\]� '� � () [\ - -"J ' . � (:) - t 1\ ;:i .�L\. :с;.':'\ /�· \ � �у D 5:: 3oL r· o ",г\.. _ <\ - 1 !'\ F (.:; �� r,A, Vо\иг --; ' I ! ю�\17� ,_.. ..>; О'\fч, � '<" Со �1-c··CJ�8 3 l;cb= 'ч \-1 ,Ц-Ьо"� ) 1м.F 1 jVl,r.;· !:::t):::�.'J V\_oci (t!'Q \� \ t--', � ED :::. \ 1""> . ., Е::А f' �-. ' {V\, ,v,<'-"'°'� МдS,::,- \ {п S уч·'( � �1/Q ..- if\-!J �-'v::,�1,gls -tJ о � \'<:; '\от ��\ 'f,,O '/,- ,: �С:,� �-S 8. 1 н ;С.,н. � 1-1 �ч , �ot С'.· чt� � "' " 'f. 3. KCI ;, . \ .;;.� ¼."- )1- Attractive Forces (IMF) Polar/ Nonpolar molecule Draw the molecule С; Lo �с: -d ч 1 � , What method would you use to determine the strongest intermolecular forces between а group of nonpolar molecules such as F2, Cl2, 12? i ,::, • F' IJ , "1 __ 1,-_ ••,\. \ { i) i а- ➔ � С\.,� \ �Q \)(}с,,, What method would уьt use to determine ihe strongest intermolecuTar forces betw�n а group of i 0 polar molecules such as water, ammonia and salt? .\ 1 о\ r "\/ (', ·-. j\'-._ \-"(J"'(_:\,.., \V\ � Т ;;. ➔ l i\i\ :,Ji"-.Y..,•j•·"·~'<._. 1, r, , , \) ,.•.'_j\•� • \~ �v � г ,q.c)-,1.5)/i \ 7 r'\ �:- . J sц 1. s . ' � а. Under which conditions of temperature and pressure do real gases "act" MOST Iike ide al gases? Explain why. ..L . --'? 1-\- L � ➔ � Ov� ·'"'7 \' \?� _,, Lo oq,cvd. , Ь. Under which conditions of temperature and pressure do real gases "act" LEAST like ideal _gases? Explain why. _l__J_ Lo ·rsм. Р - S I о w � � au:тca,_z 1+, pu'\,QW - � � -cd.lA_ct_(_ с. Which two real gases MOST resemЫe ideal gases? WНУ? 1+ д of li t {�\ &а;О What two properties does Boyle's Law relate? V { Describe the relationship between these two properties. Pt \[ i �v��ck Ь. What is the formula to use when solving Boyle's Law proЫems? ·v, � , -=-- ?(j \J в-- а,\. What two properties does Ch rles' Law relate? (KELV\ a а. Describe the rel a tionship between these two properties. tRi= S LorJS.TA,vr ✓t·,t ula to use when solving Charles' law proЫems? j ___J_. � \ --· с. What happens to t!e volu;;:;t;;'вf an ideal gas at О Kelvin? Ь. What is the fo J� Could this happen to а real gas? Why or why not? v 1\1\ -J т

Related Documents

Apply Valence Bond Theory to Write Hybridization and Bonding Schemes

Dimensional Analysis - Stoichiometry and Mass to Mass Conversions

Molecular Orbital Diagram for Diatomic Ion

Determining Molecular Formula from Experimental Data

Drawing Lewis Structures, Resonance and Formal Charge for Phosphate

Drawing Lewis Structures, Exceptions, XeF6, Xenon Hexafluoride

Draw Lewis Dot Structures for Covalent Compounds

Dimensional Analysis: Limiting Reagent, Theoretical Yield

Dimensional Analysis, Mass of Element to Volume of Compound

Dimensional Analysis Ions to Mass

The Mole and Molar Mass

Determining Molecular Formula Using Combustion Analysis

Applying Molecular Orbital Theory

Apply VSEPR Theory to Predict Molecular Geometry

Compare the Solid, Liquid and Gas Phases at the Molecular Level

Bond Energies and Bond Lengths

Balancing Chemical Equations By Ions

Balancing Chemical Equations by Atoms

Balancing a Combustion Reaction by Atom

Balancing a Chemical Reaction with All Ionic Compounds by Ions

Unit 1: States of Matter and Intermolecular Forces

of 6

0/0

Recommended Documents

TOP DOCUMENT

Cell Division Gizmo Answers
High School High School Chemistry
Lecture Note

TOP DOCUMENT

Chemistry Unit 7 Review Answer Key
High School High School Chemistry
Answer Key

TOP DOCUMENT

Student Exploration Water Pollution
High School High School Chemistry
Lab

⏰ Deadline pressure?
Get your assignment done in just 3 hours. Quick, easy, and available 24/7.

Assignment – What is a Mole?
High School High School Chemistry
Lecture Note

New Documents from this Course

Net Ionic Equations
High School High School Chemistry
Answer Key

Nuclear Chemistry – Alpha, Beta, and Gamma Decay Practice
High School High School Chemistry
Answer Key

Darwins Natural Selection
High School High School Chemistry
Answer Key

Kami Export - Unit 5 Exam
High School High School Chemistry
Answer Key

Electrons Notes
High School High School Chemistry
Lecture Note

IB Chemistry: Buffer Solutions
High School High School Chemistry
Lecture Note

The Citric Acid Cycle
High School High School Chemistry
Lecture Note

Atoms and Elements Notes
High School High School Chemistry
Lecture Note

Acids, Bases, Salts
High School High School Chemistry
Lecture Note

Determination of Salivary Amylase
High School High School Chemistry
Lab

Determination of Blood Sugar
High School High School Chemistry
Lab

Determination of Blood Creatinine
High School High School Chemistry
Lab

Fair Use Policy

EduBirdie considers academic integrity to be the essential part of the learning process and does not support any violation of the academic standards. Should you have any questions regarding our Fair Use Policy or become aware of any violations, please do not hesitate to contact us via support@edubirdie.com.

Popular Services

Essay writing service

Pay someone to do my homework

Do my assignment for me

Pay for essay

Essay writers for hire

Write my research paper

Do my homework

Personal statement writing service

Study Resources

Essay Examples

Blog

Study Notes

About Us

How it works?

Testimonials

FAQ

Money back guarantee

Contact us

support@edubirdie.com

+3 (595) 691 8356

+1 (888) 337 5415

For press

Press and media

Brand assets

Local sites

We accept

2024 © EduBirdie.com. All rights reserved

Privacy Policy
|
Terms of Use
|
Fair use policy

Subscription rules
|
Referral program Rules
|
Payment policy

Description

Related Documents

Want to Download This Document?

Free up your schedule!

Take 5 seconds to unlock