Chapter 8 Test Study Guide AP Chemistry 6 points DUE AT TEST (Wed., 12/13/17) Date:

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Chapter 8 Test Study Guide AP Chemistry 6 points DUE AT TEST (Wed., 12/13/17) Date:"

Transcription

1 Chapter 8 Test Study Guide Name: AP Chemistry 6 points DUE AT TEST (Wed., 12/13/17) Date: Topics to be covered on the December 13, 2017 test: bond bond energy ionic bond covalent bond polar covalent bond electronegativity (no table provided) ä bond polarity polar/dipolar/dipole moment ionic radius ionic radius trend ion (prediction of charge) cation anion isoelectronic Lewis structures duet rule octet rule (and exceptions to it) bonding pair shared pair lone pair (unshared pair) single bond double bond triple bond endothermic exothermic breaking bonds making bonds resonance delocalization VSEPR VSEPR shapes formal charge calculation of enthalpy of reaction using bond energy tables lattice energy 1) Explain the following variations in radius: (a) I - > I > I + (all have the same p + ; I + lost an e -, so p + attract electrons more and make radius smaller) (b) Ca 2+ > Mg 2+ > Be 2+ (same group; Ca 2+ has more energy levels, so valence electrons are farther from nucleus) (c) Fe > Fe 2+ > Fe 3+ (Fe 3+ has lost more electrons, so there s less repulsion and radius is smaller) 2) Place F, Br, and Br - in order of decreasing size. (Br - Br F) 3) (a) What is an isoelectronic series? (sequence of ions with the same number of e - ) (b) Which neutral atom is isoelectronic with each of the following ions? Ga 3+ (Ni) Zr 4+ (Kr) Mn 7+ (Ar) I - (Xe) Pb 2+ (Hg) 4) Identify at least two ions that have the following ground-state electron configurations: (a) [Ar] (P 3-, S 2-, Cl -, K +, Ca 2+ ) (b) [Ar]3d 5 (Fe 3+, Mn 2+ ) (c) [Kr] 5s 2 4d 10 (Sn 2+, In + ) 5) Consider S, Cl, K, and their most common ions. (a) List the atoms in terms of increasing size. (Cl S K) (b) List the ions in order of increasing size. (K + Cl - S 2- ) (c) Explain any differences in the orders of the atomic and ionic sizes. K = more energy levels, so larger than Cl or S K +, S 2-, Cl - are isoelectronic; S 2- has gained the most e -, so it is the largest because there is more electron replusion 6) For each of the following sets of atoms and ions, arrange the members in order of increasing size: (a) Se 2-, Te 2-, Se (Se < Se 2- < Te 2- ) (b) Co 3+, Fe 2+, Fe 3+ (Fe 3+ < Fe 2+ and Co 3+ < Fe 3+ )

2 [I WILL NOT ASK ONE THIS DIFFICULT] (c) Ca, Ti 4+, Sc 3+ (Ti 4+ < Sc 3+ < Ca) (d) Be 2+, Na +, Ne (Be 2+ < Na + < Ne) 7) Does the lattice energy of an ionic solid increase or decrease (a) as the charges on the ions increase? (increase) (b) as the sizes of the ions increase? (decrease) (c) Arrange the following substances according to their expected lattice energies (from lowest lattice energy to highest): MgS, KI, GaN, LiBr (KI, LiBr, MgS, GaN) 8) Explain the following trends in lattice energy: (a) NaCl > RbBr > CsBr (NaCl = smallest ions) (b) BaO > KF (BaO = higher charges than KF) (c) SrO > SrCl 2 (SrO = higher charges than Sr 2+ and Cl - ) 9) Using only a periodic table, select the most electronegative atom in each of the following sets (then check yourself with a table): a) Na, Mg, K, Ca b) Be, B, C, Si c) P, S, As, Se d) Zn, Ge, Ga, As 10) Arrange the following sets of bonds in order of increasing polarity: a) C F, O F, Be F b) O Cl, S Br, C P (O F, C F, Be F) (S Br, C P, O Cl) c) S C, B F, N O (S C, N O, B F) 11) Rank the following bonds in order of INCREASING ionic character (from most covalent to most ionic): N O, Ca O, C F, Br Br, K F (Br Br, N O, C F, Ca O, K F) 12) Draw the Lewis structures for each of the following. Then predict the bond angles and VSEPR shape: a) HF g) N 2 l) NH 3 r) CH 4 linear 180 linear 180 trigonal pyramid tetrahedral

3 b) CF 4 h) NO + m) HCN (central atom is carbon) (tetrahedral like [:N O:] + H-C N: methane) linear 180 linear 180 c) PH 3 i) CHCl 3 n) NH 4 + s) O 2 trigonal pyramid 107 tetrahedral tetrahedral linear 180 d) H 2 CO (central atom is carbon) o) SeF 2 t) HBr trigonal planar 120 bent linear 180 e) POCl 3 j) SO 4 2- p) XeO 4 u) ClO 4 - tetrahedral tetrahedral tetrahedral tetrahedral f) PO 4 3- k) SO 3 2- q) ClO 2 - r) PCl 5 tetrahedral trigonal pyramid bent trigonal bipyramidal s) SeCl 6 t) ICl 5 u) TeF 4 v) PCl 3 octahedral square pyramid see-saw trigonal pyramid 13) Write the electron configurations for a) the cations Sr 2+, Cs +, Pb 2+, and In + [Kr] [Xe] [Xe]6s 2 5d 10 [Kr]5s 2 4d 10 b) the anions P 3-, Br -, and S 2- [Ar] [Kr] [Ar]

4 14) Which of the following ions have noble gas electron configurations? a) Fe 2+, Fe 3+, Sc 3+, Co 3+ b) Tl +, Te 2-, Cr 3+ c) Pu 4+, Ce 4+, Ti 4+ d) Ba 2+, Pt 2+, Mn 2+ 15) Which noble gas has the same electron configuration as each of the ions in the following compounds? a) cesium sulfide b) strontium fluoride [Xe] [Ar] [Kr] [Ne] c) calcium nitride d) aluminum bromide [Ar] [Ne] [Ne] [Kr] 16) For each of the following groups, place the atoms and ions in order of DECREASING size: a) Cu, Cu +, Cu 2+ b) Ni 2+, Pd 2+, Pt 2+ (Cu > Cu + > Cu 2+ ) (Pt 2+ > Pd 2+ > Ni 2+ ) c) O, O -, O 2- d) La 3+, Eu 3+, Gd 3+, Yb 3+ (O 2- > O - > O) (La 3+ > Eu 3+ > Gd 3+ > Yb 3+ ) e) Te 2-, I -, Cs +, Ba 2+, La 3+ (Te 2- > I - > Ba 2+ > La 3+ ) 17) Predict the empirical formulas of the ionic compounds formed from the following pairs of elements. a) Al and F b) K and S c) Y and O d) Mg and N AlF 3 K 2 S YO or Y 2 O 3 Mg 3 N 2 d) Ba and F e) Cs and Cl f) Li and N g) Al and O BaF 2 CsCl Li 3 N Al 2 O 3 18) Use the bond energy tables to estimate ÄH for each of the following reactions in the gas phase: (a) H 2 S + 3 F 2 > SF HF [-1282 kj] (b) C 2 H 2 + 5/2 O 2 > 2 CO 2 + H 2 O [-1228 kj] 19) Use the bond energy tables to predict ÄH for the isomerization of methyl isocyanide to acetonitrile: CH 3 N C (g) > CH 3 C N (g) [-42 kj] 20) Use bond energies to predict ÄH for the combustion of ethyl alcohol. [-1276 kj] CH 3 CH 2 OH + 3 O 2 > 2 CO H 2 O (first draw structures, then break and make bonds!) 21) Use bond energies to estimate ÄH for the following reaction: H 2 O 2 (aq) + CH 3 OH (aq) -----> H 2 CO (aq) + 2 H 2 O ( ) [-295 kj]

5 22) (a) What is the trend in electronegativity going from left to right in a row on the periodic table? (increases) (b) How do electronegativity values generally vary going down a column on the periodic table? (decrease) (c) How do the periodic trends of first ionization energy and atomic radius relate to electronegativity? (FIE follows EN trend, atomic radius is opposite EN trend) 23) What is the difference between an ionic bond and a polar covalent bond? (ionic = transfer of electron, most polar; polar covalent = unequal sharing of e - ) 24) Which has the largest dipole moment, an ionic bond, a covalent bond, or a polar covalent bond? (ionic) 25) p. 398 # 119 (see book for answer) 26) p. 397 #101 (see book for answer) 27) p. 397 #92 (resonance) 28) p. 393 #25 (see book for answer) 29) p. 393 #26 c = true; A = XeCl 2 is linear; B = SO 2 angle is larger than SCl 2 but smaller than CS 2 ; D = MINIMIZE repulsions! 30) p. 395 #61 (see book for answer) 31) p. 402-A 1) C 2) D 3) A 4) B 8) D 11) A 12) A 13) B

Homework #6 Chapter 13 Bonding: General Concepts

Homework #6 Chapter 13 Bonding: General Concepts Homework #6 Chapter 13 Bonding: General Concepts 17. Electronegativity increases from left to right across periods and from low to high along groups. a) C

More information

Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.

Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Review: Comparison of ionic and molecular compounds Molecular compounds Ionic

More information

Bonding/Lewis Dots Lecture Page 1 of 12 Date. Bonding. What is Coulomb's Law? Energy Profile: Covalent Bonds. Electronegativity and Linus Pauling

Bonding/Lewis Dots Lecture Page 1 of 12 Date. Bonding. What is Coulomb's Law? Energy Profile: Covalent Bonds. Electronegativity and Linus Pauling Bonding/Lewis Dots Lecture Page 1 of 12 Date Bonding What is Coulomb's Law? Energy Profile: Covalent Bonds Electronegativity and Linus Pauling 2.1 H 1.0 Li 0.9 Na 0.8 K 0.8 Rb 0.7 Cs 0.7 Fr 1.5 Be 1.2

More information

1. What is the phenomenon that occurs when certain metals emit electrons when illuminated by particular wavelengths of light? a.

1. What is the phenomenon that occurs when certain metals emit electrons when illuminated by particular wavelengths of light? a. CHEMISTRY 123-07 Midterm #3 solution key December 02, 2010 Statistics: Average: 77 p (77%); Highest: 100 p (100%); Lowest: 33 p (33%) Number of students performing at or above average: 54 (52%) Number

More information

M10/4/CHEMI/SPM/ENG/TZ2/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES

M10/4/CHEMI/SPM/ENG/TZ2/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES M10/4/CHEMI/SPM/ENG/TZ/XX+ 106116 CHEMISTRY standard level Paper 1 Wednesday 1 May 010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer

More information

bond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction

bond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction bond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction ionic compound- a metal reacts with a nonmetal Ionic bonds form when an atom that

More information

Review for Chapter 4: Structures and Properties of Substances

Review for Chapter 4: Structures and Properties of Substances Review for Chapter 4: Structures and Properties of Substances You are responsible for the following material: 1. Terms: You should be able to write definitions for the following terms. A complete definition

More information

Chapter 8. Bonding: General Concepts

Chapter 8. Bonding: General Concepts Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.2 Electronegativity 8.3 Bond Polarity and Dipole Moments 8.4 Ions: Electron Configurations and Sizes 8.5 Energy

More information

PERIODIC TABLE OF THE ELEMENTS

PERIODIC TABLE OF THE ELEMENTS Useful Constants and equations: K = o C + 273 Avogadro's number = 6.022 x 10 23 d = density = mass/volume R H = 2.178 x 10-18 J c = E = h = hc/ h = 6.626 x 10-34 J s c = 2.998 x 10 8 m/s E n = -R H Z 2

More information

Chapter 8. Bonding: General Concepts

Chapter 8. Bonding: General Concepts Chapter 8 Bonding: General Concepts Chapter 8 Questions to Consider What is meant by the term chemical bond? Why do atoms bond with each other to form compounds? How do atoms bond with each other to form

More information

Draw the Lewis Structures. Unit 4 Bonding II Review 12/15/ ) PBr 3 4) NO 2) N 2 H 2 5) C 2 H 4. 3) CH 3 OH 6) HBr. Ionic. Covalent.

Draw the Lewis Structures. Unit 4 Bonding II Review 12/15/ ) PBr 3 4) NO 2) N 2 H 2 5) C 2 H 4. 3) CH 3 OH 6) HBr. Ionic. Covalent. Unit 4 Bonding II Review Unit 4 Bonding II Determine the type of bond (, or Metallic) in the following compounds: Compound Bond Type Compound Bond Type NaCl CO FeNi SiS 2 Metallic NCl 3 PF 3 CaCl 2 Fe

More information

Name Date Class STUDY GUIDE FOR CONTENT MASTERY. covalent bond molecule sigma bond exothermic pi bond

Name Date Class STUDY GUIDE FOR CONTENT MASTERY. covalent bond molecule sigma bond exothermic pi bond Covalent Bonding Section 9.1 The Covalent Bond In your textbook, read about the nature of covalent bonds. Use each of the terms below just once to complete the passage. covalent bond molecule sigma bond

More information

Chemistry 121: Topic 4 - Chemical Bonding Topic 4: Chemical Bonding

Chemistry 121: Topic 4 - Chemical Bonding Topic 4: Chemical Bonding Topic 4: Chemical Bonding 4.0 Ionic and covalent bonds; Properties of covalent and ionic compounds 4.1 Lewis structures, the octet rule. 4.2 Molecular geometry: the VSEPR approach. Molecular polarity.

More information

All chemical bonding is based on the following relationships of electrostatics: 2. Each period on the periodic table

All chemical bonding is based on the following relationships of electrostatics: 2. Each period on the periodic table UNIT VIII ATOMS AND THE PERIODIC TABLE 25 E. Chemical Bonding 1. An ELECTROSTATIC FORCE is All chemical bonding is based on the following relationships of electrostatics: The greater the distance between

More information

Chapter 7. Chemical Bonding I: Basic Concepts

Chapter 7. Chemical Bonding I: Basic Concepts Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely

More information

7. How many unpaired electrons are there in an atom of tin in its ground state? 2

7. How many unpaired electrons are there in an atom of tin in its ground state? 2 Name period AP chemistry Unit 2 worksheet 1. List in order of increasing energy: 4f, 6s, 3d,1s,2p 1s, 2p, 6s, 4f 2. Explain why the effective nuclear charge experienced by a 2s electron in boron is greater

More information

Chapter 10: Modern Atomic Theory and the Periodic Table. How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation

Chapter 10: Modern Atomic Theory and the Periodic Table. How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation Chapter 10: Modern Atomic Theory and the Periodic Table How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation Electromagnetic (EM) radiation is a form of energy that exhibits

More information

CHAPTER 12 CHEMICAL BONDING

CHAPTER 12 CHEMICAL BONDING Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 12 CHEMICAL BONDING Day Plans for the day Assignment(s) for the day 1 Begin Chapter

More information

Chapter 8. Bonding: General Concepts

Chapter 8. Bonding: General Concepts Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.3 Bond Polarity and Dipole Moments 8.5 Energy Effects in Binary Ionic Compounds 8.6 Partial Ionic Character

More information

CHAPTER 8 BONDING: GENERAL CONCEPTS

CHAPTER 8 BONDING: GENERAL CONCEPTS Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 8 BONDING: GENERAL CONCEPTS Day Plans for the day Assignment(s)

More information

Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas.

Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas. CHEMICAL BONDING Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas. 1.Electrons can be from one atom to another forming. Positive ions (cations) are formed when

More information

NAME: FIRST EXAMINATION

NAME: FIRST EXAMINATION 1 Chemistry 64 Winter 1994 NAME: FIRST EXAMINATION THIS EXAMINATION IS WORTH 100 POINTS AND CONTAINS 4 (FOUR) QUESTIONS THEY ARE NOT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIONS AND ALLOCATE YOUR

More information

Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts

Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts Types of Chemical Bonds Information about the strength of a bonding interaction is obtained by measuring the bond energy, which is the energy

More information

CHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols

CHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols CHEMICAL BONDING Chemical Bonds Lewis Symbols Octet Rule whenever possible, valence electrons in covalent compounds distribute so that each main-group element is surrounded by 8 electrons (except hydrogen

More information

Chapter Eight. p328. Bonding: General Concepts

Chapter Eight. p328. Bonding: General Concepts Chapter Eight p328 Bonding: General Concepts 1 Contents 8-1 Types of Chemical Bonds p330 Coulomb s law The energy of interaction between a pair of ions can be calculated using Coulomb s law: E 19 Q1Q 2

More information

What is a Bond? Chapter 8. Ionic Bonding. Coulomb's Law. What about covalent compounds?

What is a Bond? Chapter 8. Ionic Bonding. Coulomb's Law. What about covalent compounds? Chapter 8 What is a Bond? A force that holds atoms together. Why? We will look at it in terms of energy. Bond energy- the energy required to break a bond. Why are compounds formed? Because it gives the

More information

The Periodic Table. Periodic Properties. Can you explain this graph? Valence Electrons. Valence Electrons. Paramagnetism

The Periodic Table. Periodic Properties. Can you explain this graph? Valence Electrons. Valence Electrons. Paramagnetism Periodic Properties Atomic & Ionic Radius Energy Electron Affinity We want to understand the variations in these properties in terms of electron configurations. The Periodic Table Elements in a column

More information

CHEM 172 EXAMINATION 1. January 15, 2009

CHEM 172 EXAMINATION 1. January 15, 2009 CHEM 17 EXAMINATION 1 January 15, 009 Dr. Kimberly M. Broekemeier NAME: Circle lecture time: 9:00 11:00 Constants: c = 3.00 X 10 8 m/s h = 6.63 X 10-34 J x s J = kg x m /s Rydberg Constant = 1.096776 x

More information

Polar bonds, polar molecules and the shape of molecules.

Polar bonds, polar molecules and the shape of molecules. Chapter 3 Polar bonds, polar molecules and the shape of molecules. Polar and non-polar bonds In homonuclear diatomic molecules such as H 2 or Cl 2 electrons are shared equally between equal atoms. The

More information

1. Following Dalton s Atomic Theory, 2. In 1869 Russian chemist published a method. of organizing the elements. Mendeleev showed that

1. Following Dalton s Atomic Theory, 2. In 1869 Russian chemist published a method. of organizing the elements. Mendeleev showed that 20 CHEMISTRY 11 D. Organizing the Elements The Periodic Table 1. Following Dalton s Atomic Theory, By 1817, chemists had discovered 52 elements and by 1863 that number had risen to 62. 2. In 1869 Russian

More information

Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules

Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Fructose Water Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Carbon Dioxide Ammonia Title and Highlight TN Ch 10.1 Topic: EQ: Right Side NOTES

More information

Made the FIRST periodic table

Made the FIRST periodic table Made the FIRST periodic table 1869 Mendeleev organized the periodic table based on the similar properties and relativities of certain elements Later, Henri Moseley organized the elements by increasing

More information

CHAPTER 8 BONDING: GENERAL CONCEPTS Ionic solids are held together by strong electrostatic forces that are omnidirectional.

CHAPTER 8 BONDING: GENERAL CONCEPTS Ionic solids are held together by strong electrostatic forces that are omnidirectional. CAPTER 8 BDIG: GEERAL CCEPTS 1 CAPTER 8 BDIG: GEERAL CCEPTS Questions 15. a. This diagram represents a polar covalent bond as in. In a polar covalent bond, there is an electron rich region (indicated by

More information

CHEM 130 Exp. 8: Molecular Models

CHEM 130 Exp. 8: Molecular Models CHEM 130 Exp. 8: Molecular Models In this lab, we will learn and practice predicting molecular structures from molecular formulas. The Periodic Table of the Elements IA 1 H IIA IIIA IVA VA VIA VIIA 3 5

More information

CHE 105 Spring 2018 Exam 3

CHE 105 Spring 2018 Exam 3 CHE 105 Spring 2018 Exam 3 Your Name: Your ID: Question #: 1 Which three statements about energy are true? A. Energy cannot be created or destroyed. B. The three forms of energy are kinetic, potential,

More information

Chemical bonding is the combining of elements to form new substances.

Chemical bonding is the combining of elements to form new substances. Name Covalent Bonding and Nomenclature: Unit Objective Study Guide Class Period Date Due 1. Define chemical bonding. What is chemical bonding? Chemical bonding is the combining of elements to form new

More information

CHEMISTRY Midterm #3 November 27, 2007

CHEMISTRY Midterm #3 November 27, 2007 Name: The total number of points in this exam is 100. CHEMISTRY 123-01 Midterm #3 November 27, 2007 PART I: MULTIPLE CHOICE (Each multiple choice question has a 2-point value). Mass of electron = 9.11

More information

properties) YOU NEED TO KNOW THESE!!!!

properties) YOU NEED TO KNOW THESE!!!! 4.2.A ReIntro to Bonding I Pledge : ( Initial ) DON T FORGET WHAT THIS REPRESENTS. Instructions: Provide a response for each question that is well thought out, satisfies the prompt, is clearly explained,

More information

Name: Practice Packet. Regents Chemistry: Dr. Shanzer. Chapter 9: Chemical Bonding.

Name: Practice Packet. Regents Chemistry: Dr. Shanzer. Chapter 9: Chemical Bonding. Name: Regents Chemistry: Dr. Shanzer Practice Packet Chapter 9: Chemical Bonding http://drshanzerchemistry.weebly.com 1 Chemical Bonding Objectives Describe the 2 major types of chemical bonds in terms

More information

Test Review # 4. Chemistry: Form TR4.11A

Test Review # 4. Chemistry: Form TR4.11A Chemistry: Form TR4.11 REVIEW Name Date Period Test Review # 4 Bonding. The electrons of one atom are attracted to the protons of another. When atoms combine, there is a tug of war over the valence electrons.

More information

M11/4/CHEMI/SPM/ENG/TZ2/XX CHEMISTRY STANDARD LEVEL PAPER 1. Monday 9 May 2011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES

M11/4/CHEMI/SPM/ENG/TZ2/XX CHEMISTRY STANDARD LEVEL PAPER 1. Monday 9 May 2011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES M11/4/CHEMI/SPM/ENG/TZ/XX 116116 CHEMISTRY STANDARD LEVEL PAPER 1 Monday 9 May 011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer

More information

Chemistry 101 Chapter 9 CHEMICAL BONDING. Chemical bonds are strong attractive force that exists between the atoms of a substance

Chemistry 101 Chapter 9 CHEMICAL BONDING. Chemical bonds are strong attractive force that exists between the atoms of a substance CHEMICAL BONDING Chemical bonds are strong attractive force that exists between the atoms of a substance Chemical Bonds are commonly classified into 3 types: 1. IONIC BONDING Ionic bonds usually form between

More information

C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE INSTR : FİLİZ ALSHANABLEH

C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE INSTR : FİLİZ ALSHANABLEH C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE The Ionic Bond Formation of Ions The

More information

Bonding. Honors Chemistry 412 Chapter 6

Bonding. Honors Chemistry 412 Chapter 6 Bonding Honors Chemistry 412 Chapter 6 Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Types of Bonds Ionic Bonds Force of attraction

More information

Unit Six --- Ionic and Covalent Bonds

Unit Six --- Ionic and Covalent Bonds Unit Six --- Ionic and Covalent Bonds Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals Valence Electrons Electrons in the highest occupied energy level of an element s atoms Examples

More information

8. Relax and do well.

8. Relax and do well. CHEM 1225 Exam I John I. Gelder February 4, 1999 Name KEY TA's Name Lab Section Please sign your name below to give permission to post your course scores on homework, laboratories and exams. If you do

More information

Funsheet 8.0 [SCIENCE 10 REVIEW] Gu 2015

Funsheet 8.0 [SCIENCE 10 REVIEW] Gu 2015 Funsheet 8.0 [SCIENCE 10 REVIEW] Gu 2015 1. Fill in the following tables. Symbol # # protons electrons # neutrons Atomic number Mass Number Atomic Mass Charge 56 54 83 18 16 32 35 47 1 19 40 1+ 92 241

More information

Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond

Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H

More information

"What Do I Remember From Introductory Chemistry?" - A Problem Set

What Do I Remember From Introductory Chemistry? - A Problem Set 1 "What Do I Remember From Introductory Chemistry?" - A Problem Set These problems review a portion of the material from introductory chemistry that you should be very familiar with. 1. The electron configuration

More information

We study bonding since it plays a central role in the understanding of chemical reactions and understanding the chemical & physical properties.

We study bonding since it plays a central role in the understanding of chemical reactions and understanding the chemical & physical properties. AP Chapter 8 Notes Bonding We study bonding since it plays a central role in the understanding of chemical reactions and understanding the chemical & physical properties. Chemical Bond: holding atoms together

More information

Properties of substances are largely dependent on the bonds holding the material together.

Properties of substances are largely dependent on the bonds holding the material together. Basics of Chemical Bonding AP Chemistry Lecture Outline Properties of substances are largely dependent on the bonds holding the material together. Basics of Bonding A chemical bond occurs when atoms or

More information

Chemical Bonding polarity & Dipole Moments. Chapter 8 Part III

Chemical Bonding polarity & Dipole Moments. Chapter 8 Part III Chemical Bonding polarity & Dipole Moments Chapter 8 Part III Exercise Arrange the following bonds from most to least polar: a) N F O F C F b) C F N O Si F c) Cl Cl B Cl S Cl Exercise a) C F, N F, O F

More information

Honors Chemistry - Unit 4 Bonding Part I

Honors Chemistry - Unit 4 Bonding Part I Honors Chemistry - Unit 4 Bonding Part I Unit 4 Packet - Page 1 of 8 Vocab Due: Quiz Date(s): Test Date: UT Quest Due: Bonding Vocabulary: see separate handout assignment OBJECTIVES: Chapters 4-8 Be able

More information

M09/4/CHEMI/SPM/ENG/TZ1/XX+ CHEMISTRY. Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES

M09/4/CHEMI/SPM/ENG/TZ1/XX+ CHEMISTRY. Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES M09/4/CHEMI/SPM/ENG/TZ1/XX+ 22096110 CHEMISTRY standard level Paper 1 Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so.

More information

A DOT STRUCTURE FOR A LARGER MOLECULE ETHANOL! Count valence electrons

A DOT STRUCTURE FOR A LARGER MOLECULE ETHANOL! Count valence electrons 212 A DOT STRUCTURE FOR A LARGER MOLECULE Count valence electrons Pick central atom and draw skeletal structure - central atom is usually the one that needs to gain the most electrons! - skeletal structure

More information

Chapter 7 Chemical Bonding

Chapter 7 Chemical Bonding Chapter 7 Chemical Bonding 7.1 Ionic Bonding Octet rule: In forming compounds atoms lose, gain or share electrons to attain a noble gas configuration with 8 electrons in their outer shell (s 2 p 6 ), except

More information

Chapter 7. Ionic & Covalent Bonds

Chapter 7. Ionic & Covalent Bonds Chapter 7 Ionic & Covalent Bonds Ionic Compounds Covalent Compounds 7.1 EN difference and bond character >1.7 = ionic 0.4 1.7 = polar covalent 1.7 Electrons not shared at

More information

CHAPTER 12: CHEMICAL BONDING

CHAPTER 12: CHEMICAL BONDING CHAPTER 12: CHEMICAL BONDING Problems: 1-26, 27c, 28, 33-34, 35b, 36(a-c), 37(a,b,d), 38a, 39-40, 41-42(a,c), 43-58, 67-74 12.1 THE CHEMICAL BOND CONCEPT chemical bond: what holds atoms or ions together

More information

Solutions and Ions. Pure Substances

Solutions and Ions. Pure Substances Class #4 Solutions and Ions CHEM 107 L.S. Brown Texas A&M University Pure Substances Pure substance: described completely by a single chemical formula Fixed composition 1 Mixtures Combination of 2 or more

More information

Name Unit Three MC Practice March 15, 2017

Name Unit Three MC Practice March 15, 2017 Unit Three: Bonding & Molecular Geometry Name Unit Three MC Practice March 15, 2017 1. What is the hybridization of the oxygen atom in water? a) sp b) sp 2 c) sp 3 d) It is not hybridized 2. When a double

More information

Atomic Structure & Interatomic Bonding

Atomic Structure & Interatomic Bonding Atomic Structure & Interatomic Bonding Chapter Outline Review of Atomic Structure Atomic Bonding Atomic Structure Atoms are the smallest structural units of all solids, liquids & gases. Atom: The smallest

More information

Chapter 8. Basic Concepts of Chemical Bonding

Chapter 8. Basic Concepts of Chemical Bonding Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds An attractive force that holds two atoms together in a more complex unit Three basic types of bonds Ionic Electrons are transferred from one

More information

51. Pi bonding occurs in each of the following species EXCEPT (A) CO 2 (B) C 2 H 4 (C) CN (D) C 6 H 6 (E) CH 4

51. Pi bonding occurs in each of the following species EXCEPT (A) CO 2 (B) C 2 H 4 (C) CN (D) C 6 H 6 (E) CH 4 Name AP Chemistry: Bonding Multiple Choice 41. Which of the following molecules has the shortest bond length? (A) N 2 (B) O 2 (C) Cl 2 (D) Br 2 (E) I 2 51. Pi bonding occurs in each of the following species

More information

Chapter 8. Bonding: General Concepts. Copyright 2017 Cengage Learning. All Rights Reserved.

Chapter 8. Bonding: General Concepts. Copyright 2017 Cengage Learning. All Rights Reserved. Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents (8.1) (8.2) (8.3) (8.4) (8.5) (8.6) (8.7) (8.8) Types of chemical bonds Electronegativity Bond polarity and dipole moments Ions: Electron

More information

Subtopic 4.2 MOLECULAR SHAPE AND POLARITY

Subtopic 4.2 MOLECULAR SHAPE AND POLARITY Subtopic 4.2 MOLECULAR SHAPE AND POLARITY 1 LEARNING OUTCOMES (covalent bonding) 1. Draw the Lewis structure of covalent molecules (octet rule such as NH 3, CCl 4, H 2 O, CO 2, N 2 O 4, and exception to

More information

Chemical Bonding AP Chemistry Ms. Grobsky

Chemical Bonding AP Chemistry Ms. Grobsky Chemical Bonding AP Chemistry Ms. Grobsky What Determines the Type of Bonding in Any Substance? Why do Atoms Bond? The key to answering the first question are found in the electronic structure of the atoms

More information

(FIRST) IONIZATION ENERGY

(FIRST) IONIZATION ENERGY 181 (FIRST) IONIZATION ENERGY - The amount of energy required to remove a single electron from the outer shell of an atom. - Relates to reactivity for metals. The easier it is to remove an electron, the

More information

IB Chemistry. Chapter 4.1

IB Chemistry. Chapter 4.1 IB Chemistry Chapter 4.1 Chemical Bonds Atoms or ions that are strongly attached to one another Chemical bonds will form if potential energy decreases (becomes more stable) 2 Valence Electrons Valence

More information

AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts

AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy

More information

Ex. 1) F F bond in F = 0 < % covalent, no transfer of electrons

Ex. 1) F F bond in F = 0 < % covalent, no transfer of electrons #60 Notes Unit 8: Bonding Ch. Bonding I. Bond Character Bonds are usually combinations of ionic and covalent character. The electronegativity difference is used to determine a bond s character. Electronegativity

More information

13 Bonding: General Concepts. Types of chemical bonds. Covalent bonding Ex. H 2. Repulsions of nuclei and e s. Zero interaction at long distance

13 Bonding: General Concepts. Types of chemical bonds. Covalent bonding Ex. H 2. Repulsions of nuclei and e s. Zero interaction at long distance 13 Bonding: General Concepts Types of chemical bonds Covalent bonding Ex. 2 E (kj/mol) epulsions of nuclei and e s r 0 458 0.074 r (nm) - bond length Two e s shared by two s: covalent bonding Zero interaction

More information

Chemistry Standard level Paper 1

Chemistry Standard level Paper 1 M15/4/CHEMI/SPM/ENG/TZ1/XX Chemistry Standard level Paper 1 Thursday 14 May 2015 (afternoon) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all

More information

* one of these choices is not used

* one of these choices is not used IONIC BONDING REVIEW WORKSHEET Part 1 - Complete each of the following sentences by filling in the appropriate word or phrase from the list below. negative noble gas octet anion positive electrons ions

More information

Chapter 7 Chemical Bonding and Molecular Structure

Chapter 7 Chemical Bonding and Molecular Structure Chapter 7 Chemical Bonding and Molecular Structure Three Types of Chemical Bonding (1) Ionic: formed by electron transfer (2) Covalent: formed by electron sharing (3) Metallic: attraction between metal

More information

4/25/2017. VSEPR Theory. Two Electron Groups. Shapes of Molecules. Two Electron Groups with Double Bonds. Three Electron Groups.

4/25/2017. VSEPR Theory. Two Electron Groups. Shapes of Molecules. Two Electron Groups with Double Bonds. Three Electron Groups. Chapter 10 Lecture Chapter 10 Bonding and Properties of Solids and Liquids 10.3 Shapes of Molecules and Ions (VSEPR Theory) Learning Goal Predict the three-dimensional structure of a molecule or a polyatomic

More information

2. Write the electron configuration notation and the electron dot notation for each: (a) Ni atom (b) Ni 2+ ion (c) Ni 3+ ion

2. Write the electron configuration notation and the electron dot notation for each: (a) Ni atom (b) Ni 2+ ion (c) Ni 3+ ion EXTRA HOMEWORK 2A 1. Predict whether each of the following types of matter will be bonded with ionic, covalent, or metallic bonds, and identify whether each will be composed of atoms, ions, or molcules

More information

N = 727 Mean = 68% Diff T-Test P-Value SI 223 (31%) 71% No SI 504 (69%) 66% Test 2 - Letter Grade Distribution by SI Attendance

N = 727 Mean = 68% Diff T-Test P-Value SI 223 (31%) 71% No SI 504 (69%) 66% Test 2 - Letter Grade Distribution by SI Attendance CHEM 200/202 Exam 2 N = 727 Mean = 68% Diff T-Test P-Value SI 223 (31%) 71% No SI 504 (69%) 66% 5%

More information

- Some properties of elements can be related to their positions on the periodic table.

- Some properties of elements can be related to their positions on the periodic table. 179 PERIODIC TRENDS - Some properties of elements can be related to their positions on the periodic table. ATOMIC RADIUS - The distance between the nucleus of the atoms and the outermost shell of the electron

More information

Lewis Structure. Lewis Structures & VSEPR. Octet & Duet Rules. Steps for drawing Lewis Structures

Lewis Structure. Lewis Structures & VSEPR. Octet & Duet Rules. Steps for drawing Lewis Structures Lewis Structure Lewis Structures & VSEPR Lewis Structures shows how the are arranged among the atoms of a molecule There are rules for Lewis Structures that are based on the formation of a Atoms want to

More information

Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond

Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H

More information

- Some properties of elements can be related to their positions on the periodic table.

- Some properties of elements can be related to their positions on the periodic table. 179 PERIODIC TRENDS - Some properties of elements can be related to their positions on the periodic table. ATOMIC RADIUS - The distance between the nucleus of the atoms and the outermost shell of the electron

More information

ADVANCED PLACEMENT CHEMISTRY CHAPTERS 7, 8 AND 9 REVIEW QUESTIONS

ADVANCED PLACEMENT CHEMISTRY CHAPTERS 7, 8 AND 9 REVIEW QUESTIONS 1. What is the minimum wavelength (in nm) of a photon of light that can excite an electron in the hydrogen atom from the n = 1 to the n = 8 energy level? 2. A carbonoxygen double bond in a certain organic

More information

AP CHEMISTRY: BONDING THEORIES REVIEW KEY p. 1

AP CHEMISTRY: BONDING THEORIES REVIEW KEY p. 1 AP CHEMISTRY: BONDING THEORIES REVIEW KEY p. 1 1) a) O-H PC b) Cs-Cl I c) H-Cl PC d) Br-Br NPC 2) differences in electronegativity determines amount of ity O3 0, P8 0, NO.5, CO2 1.0, CH4.4, H2S.4 answer

More information

Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies &

Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies & Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies & electronegativity The Periodic Table What is the periodic

More information

Chapter 9: Chemical Bonding I: Lewis Theory. Lewis Theory: An Overview

Chapter 9: Chemical Bonding I: Lewis Theory. Lewis Theory: An Overview Chapter 9: Chemical Bonding I: Lewis Theory Dr. Chris Kozak Memorial University of ewfoundland, Canada Lewis Theory: An verview Valence e - play a fundamental role in chemical bonding. e - transfer leads

More information

25 Mn Ni Co Rh Fe Ru Os Uns (262) Une (266) 195.

25 Mn Ni Co Rh Fe Ru Os Uns (262) Une (266) 195. 1 Chem 64 Solutions to Problem Set #1, REVIEW 1. AO n l m 1s 1 0 0 2s 2 0 0 2p 2 1 1,0,1 3d 3 2 2, 1,0,1,2 4d 4 2 2, 1,0,1,2 4f 4 3 3, 2, 1,0,1,2,3 2. Penetration relates to the radial probability distribution

More information

Forming Chemical Bonds

Forming Chemical Bonds Forming Chemical Bonds Chemical Bonds Three basic types of bonds 2012 Pearson Education, Inc. Ionic Electrostatic attraction between ions. Covalent Sharing of electrons. Metallic Metal atoms bonded to

More information

(A) 1 bonding pair (B) 1 bonding pair and 1 lone pair (C) 2 bonding pairs (D) 2 bonding pairs and 2 lone pairs

(A) 1 bonding pair (B) 1 bonding pair and 1 lone pair (C) 2 bonding pairs (D) 2 bonding pairs and 2 lone pairs AP Chemistry - Problem Drill 13: Lewis Structures and VSPER No. 1 of 10 1. Lewis structure is used to model covalent bonds of a molecule or ion. Covalent bonds are a type of chemical bonding formed by

More information

MC Molecular Structures, Dipole Moments, Geometry, IMF Name: Date:

MC Molecular Structures, Dipole Moments, Geometry, IMF Name: Date: MC Molecular Structures, Dipole Moments, Geometry, IMF Name: Date: 2008 22. Which of the following is a nonpolar molecule that contains polar bonds? (A) F 2 (B) CHF 3 (C) CO 2 (D) HCl (E) NH 3 28. Which

More information

Bonding. Polar Vs. Nonpolar Covalent Bonds. Ionic or Covalent? Identifying Bond Types. Solutions + -

Bonding. Polar Vs. Nonpolar Covalent Bonds. Ionic or Covalent? Identifying Bond Types. Solutions + - Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Bonding onors Chemistry 412 Chapter 6 Types of Bonds Ionic Bonds Force of attraction

More information

Section 12: Lewis Structures

Section 12: Lewis Structures Section 12: Lewis Structures The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 12.01 Electronegativity Chemistry (5)(C) 12.02 Electron

More information

Chapter 3: Elements and Compounds. 3.1 Elements

Chapter 3: Elements and Compounds. 3.1 Elements Chapter 3: Elements and Compounds 3.1 Elements An element is a fundamental substance that cannot be broken down by chemical or physical methods to simpler substances. The 118 known elements are nature

More information

SHAPES OF EXPANDED VALENCE MOLECULES

SHAPES OF EXPANDED VALENCE MOLECULES 228 SHAPES OF EXPANDED VALENCE MOLECULES There are five atoms bonded to the central phosphorus atom, and they will attempt to get as far apart as possible from one another! The top and bottom atoms are

More information

Chemical Bonding Chapter 8

Chemical Bonding Chapter 8 Chemical Bonding Chapter 8 Get your Clicker, 2 magnets, goggles and your handouts Nov 15 6:15 PM Recall that: Ionic-Involves the transfer of electrons - forms between a metal and a nonmetal Covalent-Involves

More information

8.1 Types of Chemical Bonds List and define three types of bonding. chapter 8 Bonding General Concepts.notebook. September 10, 2015

8.1 Types of Chemical Bonds List and define three types of bonding. chapter 8 Bonding General Concepts.notebook. September 10, 2015 chapter 8 Bonding General Concepts.notebook Chapter 8: Bonding: General Concepts Mar 13 11:15 AM 8.1 Types of Chemical Bonds List and define three types of bonding. Bonds are forces that hold groups of

More information

7. Relax and do well.

7. Relax and do well. CHEM 1014 Exam III John III. Gelder November 18, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and

More information

Molecular Structure. Valence Bond Theory Overlap of atomic orbitals is a covalent bond that joins atoms together to form a molecule

Molecular Structure. Valence Bond Theory Overlap of atomic orbitals is a covalent bond that joins atoms together to form a molecule Molecular Structure Topics 3-D structure shape (location of atoms in space) Molecular Geometry Valence Bond Theory Hybrid Orbitals Multiple Bonds VSEPR (Valence Shell Electron Pair Repulsion) Valence Bond

More information

Q. No. 2 Bond formation is. Neither exothermic nor endothermic

Q. No. 2 Bond formation is. Neither exothermic nor endothermic Q. No. 1 Which combination will give the strongest ionic bond? K + and Cl - K + and O 2- Ca 2+ and Cl - Ca 2+ and O 2- In CaO, the polarizability of O 2- is very less therefore it has the maximum ionic

More information