ch1 atom [호환 모드] -...

1.1

일반화학 (심화반)강의개요

담당교수: 문명희, 화학과 (과학관 438호)강의시간: 화 3-4, 목 3 (과학관 B126) 교재: Oxtoby저, Principles of Modern Chemistry, 6th edition재: Oxtoby저, Principles of Modern Chemistry, 6th edition

원서사용 (필수)

강의자료 pdf-file: 문명희교수홈페이지phttp://chem.yonsei.ac.kr/~mhmoon

평가방법: 중간고사 30%평가방법: 중간고사 30%

기말고사 30% 실험 15 % 연습문제풀이, 출석태도(Quiz포함) 25 % 합 계 100 %

수업및실험중어느하나라도 1/3이상결석시에는 F학점부여

Prof. Myeong Hee Moon

1.2

Syllabus y

교과목명일반화학및 실험

( 4 )학점,주당 강의( 3 )시간교 수 명 문명희

교과목명 및 실험(심화반)

( 4 )학점,주당 강의( 3 )시간실험 ( 2 )시간 소 속

이과대학화학과

학정번호 수강대상 이학계열 1학년연락처

과학관 438호연락처

과목종별 계열기초 선수과목 2123 -5634

수업목표및

물질의 근본적인 구성요소인 원자와 분자 및 화학결합의 기초적인 개념을 소개하고,물질 상태의 대한 설명으로 기체, 농축상(액체와 고체)과 용액의 물성에 대하여 심

한다 이어서 화학 응에서 평혀에 한 이해 열역학 법칙 화및개요

도 있게 공부한다. 이어서 화학 반응에서 평혀에 대한 이해로 열역학 1,2 법칙과 화학 평혀에 대하여 공부 함으로써 화학 전반에 걸친 거시적인 관점에서 일반적이고 포괄적인 지식을 습득하는 것을 목표로 한다.

기본적 강의 시간과 실험 시간 나누어 중간 사

수업

기본적으로 강의 3시간과 실험 2시간으로 나누어실시한다. 강의 3시간은 Oxtoby의 현대 일반화학(6판) 영문판을 교재로 하여 강의실에서 PowerPoint Presentation을 통해 강의를 하고 매장마다

성적평

중간고사 30%기말고사 30% 실험 15 %기타(출석, 수업참여도, 연습문제, Quiz 등)

방식 학생들의 복습을 위하여 일정 양의 과제물을 주고이를 담당조교가 평가한다. 실험 2시간은현대일반화학의 중요한 개념을 실질적으로 이해할수 있도록 화학실험실에서 실시한다

평가방법

, )25 %

합 계 100 %* 수업 및 실험 중 어느 하나라도1/3이상 결석시에는 F학점부여


수 있도록 화학실험실에서 실시한다. 1/3이상 결석시에는 F학점부여

1.3

Syllabus y

주간 월.일 내 용 요 약 주 교 재 및참고문헌 비고참 문헌

제1주 3.2∼3.8강의소개Chapter 1. The Atom in Modern Chemistry 1. Oxtoby

Principles of 제2주 3 9 3 15 Chapter 2 Chemical Formular Equations p

Modern

Chemistry

2. Cutting edge

제2주 3.9∼3.15 Chapter 2. Chemical Formular, Equations,

제3주 3.16 ∼3.22 Chapter 3. Chemical Bonding2. Cutting edge

chemistry

츨판사:

Springer

제4주 3.23∼3.29Chapter 3. Chemical BondingChapter 4. Introduction to Quantum Mechanics

제5주 3.30∼4.5Chapter 5. Quantum Mechanics & AtomicStructure Springer

Verlag 2000년

(제13주-14주

사용)

Structure

제6주 4.6∼4.12Chapter 6. Quantum Mechanics & MolecularStructure

Chapter 6 Quantum Mechanics & Molecular 사용)제7주 4.13∼4.19Chapter 6. Quantum Mechanics & Molecular

Structure, / 보 충 수 업

제8주 4.20∼4.26 중 간 고 사 (4.20∼4.26) Oxtoby (100%)


1.4

Syllabus y제9주 4.27∼5.3 Chapter 7. Bonding in Organic Molecules

제10주 5.4∼5.10Chapter 8. Bonding in Transition Metal Compounds & Coordination Complexes

제제11주 5.11∼5.17 Chapter 9. The Gaseous state

제12주 5 18∼5 24Chapter 10. Solids, Liquids, Phase

제12주 5.18∼5.24transitions

제13주 5.25∼5.31 Chapter 11. Solutions

제14주 6.1∼6.7 특강 (화, 오후7-9시,7 9시, 과학관111호)제15주 6.8∼6.14 특강


제16주 6.15~ 6.20 기 말 고 사 (6.15∼6.20)

1.5

계산기사용

시험시간에사용가능한계산기는지나치게복잡한기능시험시간에사용가능한계산기는지나치게복잡한기능을탑재한계산기의사용을제한하며간단한수학적기능의계산기사용을권장함.능의계산기사용을권장함.

추천예: sharp EL-509V, casio FX-350MS (11,500~13,000원) ( , , )

혹은 학생회관에진열되어있는제품:

casio FX-570MS, sharp EL-5120 (18000원내외) , p ( 원내외)

그외상기기종과유사한사양의전자계산기그외상기기종과유사한사양의전자계산기

Programming 기능이있는계산기사용불가


1.6

Chapter 1

The Atom inThe Atom in Modern

Chemistry


1.7

1.1 The Nature of Modern Chemistry

Chemistry: "Chem is Try"Chemistry: Chem is TryFire⇒ Alchemy⇒ ⇒ New Materials (20th)

•What is Chemistry? A + B → C + DStudy the properties of substances, their aim being to understand their reactions can transform substances into still other substances at the molecular level.

A i l l d i h l d d di: Agricultural production, helped prevent and cure manny diseases: Increased the efficiency of energy production: reduced environmental pollutionp

No other science covers as broad a range of topics as does chemistry


as does chemistry

1.8

What Do Chemists Do?


1.9

The Scientific Method

Process of Science: asking questions and making careful observations.

science as a means of knowing;raising questions,raising questions, designing experiments, gathering data, interpreting the data, drawing conclusions, raising more questionsraising more questions

: the structured way of knowing


1.10

Two Important Laws

The Law of Conservation of Matter• The Law of Conservation of Mattermatter is neither created nor destroyed in a chemical reaction but rearranged to another subchemical reaction, but rearranged to another sub.

Antonie Lavoisier (1743-1794)

Th L f C ti f E• The Law of Conservation of EnergyEnergy is neither created nor destroyed during h i l ti b t t d i t th lchemical reactions, but converted into thermal,

electrical, or mechanical energy.

(except for nuclear reactions: matter & E(except for nuclear reactions: matter & E converted into one another through Einstein Eq.

E=mc2


E=mc .

1.11

Macroscopic & Nanoscopic Methods

Electrolytic decomposition of watery p


1.121.2 Macroscopic Methods for classifying matterclassifying matter


1.13

Homogenious vs Heterogenious mixtures


1.14

Elements, Compounds, Substances


1.151.3 Indirect Evidence for the Existence of AtomsExistence of Atoms

• The Law of Conservation of Mass -matter is neither created nor destroyed in a chemical reaction.

Antonie Lavoisier (1743-1794)

• The Law of Definite Proportions -The Law of Definite Proportionsthe components of a compound are always present in the same ratio, by mass, y

Josef Louis Proust (1799)

: Water Oxygen : hydrogen = 8:1yg y g


1.16

• Dalton’s Atomic Theory -yThe theory focused attention on the valid idea that compounds are made from little bits – atoms – combining in fixed proportions

d h h i l i f hand that chemical reactions are rearrangements of these atoms.

1 Matter consists of indivisible atoms1. Matter consists of indivisible atoms2. All the atoms of a chemical element are identical in mass3. Different chemical elements have different kinds of atoms4. Atoms are indestructible5. Compound forms in small whole-number ratios from its

l t th h bi ti f diff t telements through combination of different atoms


1.17

• Law of Multiple Proportions -

If two elements combine to form more than one compound, the masses of one element that combine

f fwith a fixed mass of the other element are in the ratios of small whole numbers.


1.18

• Avogadro’s Hypothesis -

Equal volumes of different gases at the same tem. and pressure contain equal numbers of particles.


1.19

1.4 Physical Structure of Atoms

• Atom was considered the ultimate and indivisible building block of matter

At the end of19th centuryAtoms were composed of smaller elementary particls:

protons: positively chargedneutrons: neutral electrons: negatively charged


1.20

Electrons

Electrons are found in the space around the nucleus.

J.J.Thomson(1856-1940)Plum pudding model

1897


1897

1.21

Determination of Mass-to-Charge Ratio of Electron

Electric force = Magnetic force

E: electrical fieldevHeEF E: electrical fieldH: magnetic fieldDeflection downward

EFlD /21

evHeEFE ==

eEamFtlvatD eE ==== ,/ 221

LleLNet displacement E

l

L

v

l

m

eD

l

LS

e

)())((2 2==

2

lLH

SE

m

e=∴


lLHme

1.22

Millikan’s Oil droplet experiment

1906, electric charge

e = 1 59x10-19C

was measured.

e 1.59x10 C

e = 1.6021x10-19C(by modern meas )(by modern meas.)

me = 9.1093819x10-31Kg


1.23

Nucleus

In 1911, Ernest Rutherford (NZ physicist)

Rutherford’s Gold Foil Experiment


1.24

Rutherford’s Gold Foil Experiment


1.25

Mass Spectrometry & Measurement of Relative Massesof Relative Masses

221 v

mv qV qvB m= =

2 2 2 2

,2

mv qV qvB mr

m B r m B r z

= =

∴ = → =2 2q V e V

∴ = → =


1.26

Mass Spectrum


1.27

Atomic Mass

• Atomic mass is a relative scale based on 12C = exactly 12 atomic mass units

only one with integerall other elements have mass numbersall other elements have mass numbers of integers (proton 1.0073, n=1.0087)M f i t• Mass of isotopes

• Abundance of isotopes• Atomic mass is a weighted average.


1.28

Sample Problem

Chlorine consists of two isotopes: 35Cl, isotopic mass = 34.9689, abundance 75.77%; and 37Cl, isotopic mass = 36.9659, abundance 24.23%. What is the atomic mass of chlorine?

At i (34 9689 0 7577) (36 9659 0 2423)Atomic mass = (34.9689 × 0.7577)+(36.9659 × 0.2423)

= 35.45 amu


1.29

Protons, Neutrons, Isotopes

• The number of neutrons = A−Z

• Isotopes have the same atomic

number but different mass numbersnumber but different mass numbers

1 2 3H H H1 1 1H H H


1.30

1.5 Imaging Atoms, Molecules, and Chemical ReactionsChemical Reactions

Scanning Tunneling Microscopy Imaging of Atoms


Electric current passes through a single atom in the probe tip

1.31

Homework

8, 12, 16, 20, 22


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