Test Tubes General Chemistry A CH4701. This lecture:  General information  Course syllabus  Recommended texts  Relevance of this module to you.

Test Tubes General Chemistry A CH4701

This lecture:  General information  Course syllabus  Recommended texts  Relevance of this module to you

This lecture:  General information  Course syllabus  Recommended texts  Relevance of this module to you  Topic 1:- Fundamental principles  Topic 2:- Classification of matter

Lecturer Edmond Magner MS1016 Andrew McCormack MS10 Course duration1 semester

Lecturer Edmond Magner MS1016 Teresa Curtin MSG015 Course duration1 semester Class contact2 x 50 min lectures/week 1 x 2 hour lab/fortnight Assessment60% exam, 40% labs

Lecturer Edmond Magner MS1016 Teresa Curtin MSG015 Course duration1 semester Class contact2 x 50 min lectures/week 1 x 2 hour lab/fortnight Assessment60% exam, 40% labs LabsIn B3-053 MUST have white lab coat and safety specs Your first lab session will be on week 3 (B3053)

CH 4701 COURSE SYLLABUS 1. Basics  Simple characterisation of atoms + molecules  Chemical accounting: the mole  Early chemical ideas & their present day uses  Modern theories of atomic structure  Introduction to chemical bonding  The Periodic Table

CH 4701 COURSE SYLLABUS 1. Basics  Simple characterisation of atoms + molecules  Chemical accounting: the mole  Early chemical ideas & their present day uses  Modern theories of atomic structure  Introduction to chemical bonding  The Periodic Table 2. Applied chemistry  Gas laws  Electrochemistry  Chemical equilibria (solutions and acids/bases)

TEXTS & COURSE MATERIALS Essential for all:  Good set of lecture notes!

TEXTS & COURSE MATERIALS Essential for all:  Good set of lecture notes!  CH4701 Course Materials Pack: - available from UL Print Room (E1-006) reference number 3485, price €4.50

TEXTS & COURSE MATERIALS Essential for all:  Good set of lecture notes!  CH4701 Course Materials Pack: - available from UL Print Room (E1-006) reference number 3485, price €5.00 Recommended for students without Leaving Cert chem:  Chemistry: The Central Science  8th edn., by Brown, LeMay and Bursten - available UL Bookshop, price ca. €38.00 (includes multimedia CD-ROM) Some copies of other gen. chem. texts available in UL library under classification 540.

COURSE AIMS + RELEVANCE 1. "Educate"

COURSE AIMS + RELEVANCE 1. "Educate" 2. Give a basic understanding of the theory, practice and everyday applications of chemistry to non- chemists

COURSE AIMS + RELEVANCE 1. "Educate" 2. Give a basic understanding of the theory, practice and everyday applications of chemistry to non- chemists 3. Review of fundamentals for chemists

COURSE AIMS + RELEVANCE 1. "Educate" 2. Give a basic understanding of the theory, practice and everyday applications of chemistry to non- chemists 3. Review of fundamentals for chemists CHEMISTRY

COURSE AIMS + RELEVANCE 1. "Educate" 2. Give a basic understanding of the theory, practice and everyday applications of chemistry to non- chemists 3. Review of fundamentals for chemists CHEMISTRY Describes:  structure & composition of matter

COURSE AIMS + RELEVANCE 1. "Educate" 2. Give a basic understanding of the theory, practice and everyday applications of chemistry to non- chemists 3. Review of fundamentals for chemists CHEMISTRY Describes:  structure & composition of matter  changes in structure & composition

COURSE AIMS + RELEVANCE 1. "Educate" 2. Give a basic understanding of the theory, practice and everyday applications of chemistry to non- chemists 3. Review of fundamentals for chemists CHEMISTRY Describes:  structure & composition of matter  changes in structure & composition  energy involved in these changes

FUNDAMENTAL PRINCIPLES Law of conservation of energy: "Energy can be neither created nor destroyed, but may be transformed from one form to another"

FUNDAMENTAL PRINCIPLES Law of conservation of energy: "Energy can be neither created nor destroyed, but may be transformed from one form to another" Law of conservation of mass: "Mass cannot be created or destroyed. The total mass of substances involved in a physical or chemical change remains constant"

FUNDAMENTAL PRINCIPLES Law of conservation of energy: "Energy can be neither created nor destroyed, but may be transformed from one form to another" Law of conservation of mass: "Mass cannot be created or destroyed. The total mass of substances involved in a physical or chemical change remains constant" Special theory of relativity: E = mc 2, where c = velocity of light)

CLASSIFICATION OF MATTER Properties of Matter

CLASSIFICATION OF MATTER Properties of Matter Bulk (Substantive)Particulate

CLASSIFICATION OF MATTER Properties of Matter Bulk (Substantive)Particulate Physical state

CLASSIFICATION OF MATTER Properties of Matter Bulk (Substantive)Particulate Physical state Metallic character

CLASSIFICATION OF MATTER Properties of Matter Bulk (Substantive)Particulate Physical state Metallic character Physical appearance

CLASSIFICATION OF MATTER Properties of Matter Bulk (Substantive)Particulate Physical state Metallic character Physical appearance Chemical integrity

Classification by physical state: Solid (Plutonium) Liquid(Mercury) (Chlorine)Gas

Classification by metallic character: metal or non-metal?

Classification by metallic character: metal or non-metal? Classification by physical appearance: Homogeneous Heterogeneous (Ruby) (Moon rock)

Classification by chemical integrity: Matter Mixtures

Classification by chemical integrity: Matter Mixtures (Bronze) (Agate)

Classification by chemical integrity: Matter Pure substancesMixtures (Bronze) (Agate)

Classification by chemical integrity: Matter Pure substancesMixtures Elements (Bronze) (Agate) (Carbon)

Classification by chemical integrity: Matter Pure substancesMixtures Compounds Elements (Bronze) (Agate) (Carbon) (Ice)

Definitions. Mixture: contains 2 or more pure substances, which can be separated out by physical means.

Definitions. Mixture: contains 2 or more pure substances, which can be separated out by physical means. Pure substances: have a definite chemical composition and properties. They cannot be separated into simpler substances by physical means.

Definitions. Mixture: contains 2 or more pure substances, which can be separated out by physical means. Pure substances: have a definite chemical composition and properties. They cannot be separated into simpler substances by physical means. Compound: pure substance which can be further broken down by chemical means.

Definitions. Mixture: contains 2 or more pure substances, which can be separated out by physical means. Pure substances: have a definite chemical composition and properties. They cannot be separated into simpler substances by physical means. Compound: pure substance which can be further broken down by chemical means. Element: pure substance which cannot be further broken down by ordinary chemical means.

Some examples of matter classification Steam? Gas, non-metallic, homogeneous, compound.

Some examples of matter classification Steam? Gas, non-metallic, homogeneous, compound. Sugar? Solid, non-metallic, homogeneous, compound.

Some examples of matter classification Steam? Gas, non-metallic, homogeneous, compound. Sugar? Solid, non-metallic, homogeneous, compound. Air? Gas, non-metallic, homogeneous, mixture.

Some examples of matter classification Steam? Gas, non-metallic, homogeneous, compound. Sugar? Solid, non-metallic, homogeneous, compound. Air? Gas, non-metallic, homogeneous, mixture. Brass? Solid, metallic, homogeneous, mixture.

Some examples of matter classification Steam? Gas, non-metallic, homogeneous, compound. Sugar? Solid, non-metallic, homogeneous, compound. Air? Gas, non-metallic, homogeneous, mixture. Brass? Solid, metallic, homogeneous, mixture. Mars Bar? Solid, non-metallic, heterogeneous, mixture

Differences between mixtures and compounds Mixture Compound Components can be Components can not be separated by using physical techniques

Differences between mixtures and compounds Mixture Compound Components can be Components can not be separated by using physical techniques Composition is variable Composition is fixed

Differences between mixtures and compounds Mixture Compound Components can be Components can not be separated by using physical techniques Composition is variable Composition is fixed Properties are related to Properties are unlike those of its components

Table of some of the more common elements ElementSymbol HydrogenH HeliumHe CarbonC AluminiumAl

Table of some of the more common elements ElementSymbol HydrogenH HeliumHe CarbonC AluminiumAl NitrogenN OxygenO PhosphorousP IronFe

Table of some of the more common elements ElementSymbol HydrogenH HeliumHe CarbonC AluminiumAl NitrogenN OxygenO PhosphorousP IronFe CopperCu NickelNi SulphurS IodineI

http://www.ul.ie/~ces/Resources.html

The correct classifications for sea water, distilled water, brass, and helium respectively are (a)compound, element, mixture and compound (b)mixture, element, mixture and compound

The correct classifications for sea water, distilled water, brass, and helium respectively are (a)compound, element, mixture and compound (b)mixture, element, mixture and compound (c) mixture, compound, mixture and element (d) compound, element, compound and mixture (e) mixture, compound, compound and element

The correct classifications for sea water, distilled water, brass, and helium respectively are (a)compound, element, mixture and compound (b)mixture, element, mixture and compound (c) mixture, compound, mixture and element (d) compound, element, compound and mixture (e) mixture, compound, compound and element All mixtures (indicate correct statement) (a) are heterogeneous in appearance (b) contain different types of molecules

The correct classifications for sea water, distilled water, brass, and helium respectively are (a)compound, element, mixture and compound (b)mixture, element, mixture and compound (c) mixture, compound, mixture and element (d) compound, element, compound and mixture (e) mixture, compound, compound and element All mixtures (indicate correct statement) (a) are heterogeneous in appearance (b) contain different types of molecules (c) contain two or more pure substances (d) can be separated only by chemical means (e) contain more than one physical state

DIMENSIONS AND UNITS Need to provide a quantitative means of describing the universe.

DIMENSIONS AND UNITS Need to provide a quantitative means of describing the universe. 7 independent dimensions (physical quantities):

DIMENSIONS AND UNITS Need to provide a quantitative means of describing the universe. 7 independent dimensions (physical quantities): 1. Mass (m) quantity of matter in a body

DIMENSIONS AND UNITS Need to provide a quantitative means of describing the universe. 7 independent dimensions (physical quantities): 1. Mass (m) quantity of matter in a body 2. Length (l) measurement of distance

DIMENSIONS AND UNITS Need to provide a quantitative means of describing the universe. 7 independent dimensions (physical quantities): 1. Mass (m) quantity of matter in a body 2. Length (l) measurement of distance 3. Time (t) measurement of progress of an event

DIMENSIONS AND UNITS Need to provide a quantitative means of describing the universe. 7 independent dimensions (physical quantities): 1. Mass (m) quantity of matter in a body 2. Length (l) measurement of distance 3. Time (t) measurement of progress of an event 4. Thermodynamic temperature (T). “The condition of a body which determines the transfer of heat to or from that body”

DIMENSIONS AND UNITS 5. Amount of substance (n). “The number of specified entities of a pure substance”

DIMENSIONS AND UNITS 5. Amount of substance (n). “The number of specified entities of a pure substance” 6. Electric current (I): “Rate of transfer of electricity”

DIMENSIONS AND UNITS 5. Amount of substance (n). “The number of specified entities of a pure substance” 6. Electric current (I): “Rate of transfer of electricity” 7. Luminous intensity (I v ): “Rate of transfer of light energy”

DIMENSIONS AND UNITS 5. Amount of substance (n). “The number of specified entities of a pure substance” 6. Electric current (I): “Rate of transfer of electricity” 7. Luminous intensity (I v ): “Rate of transfer of light energy” Fundamental Property of Dimensions: Two physical quantities having different dimensions cannot be added, subtracted or equated.

DIMENSIONS AND UNITS 5. Amount of substance (n). “The number of specified entities of a pure substance” 6. Electric current (I): “Rate of transfer of electricity” 7. Luminous intensity (I v ): “Rate of transfer of light energy” Fundamental Property of Dimensions: Two physical quantities having different dimensions cannot be added, subtracted or equated. All other physical quantities can be expressed in terms of these fundamental dimensions

DIMENSIONS AND UNITS 5. Amount of substance (n). “The number of specified entities of a pure substance” 6. Electric current (I): “Rate of transfer of electricity” 7. Luminous intensity (I v ): “Rate of transfer of light energy” Fundamental Property of Dimensions: Two physical quantities having different dimensions cannot be added, subtracted or equated. All other physical quantities can be expressed in terms of these fundamental dimensions e.g. volume of a cube = l x l x l = l 3

DIMENSIONS AND UNITS 5. Amount of substance (n). “The number of specified entities of a pure substance” 6. Electric current (I): “Rate of transfer of electricity” 7. Luminous intensity (I v ): “Rate of transfer of light energy” Fundamental Property of Dimensions: Two physical quantities having different dimensions cannot be added, subtracted or equated. All other physical quantities can be expressed in terms of these fundamental dimensions e.g. volume of a cube = l x l x l = l 3 velocity = distance/ time = l/t

Units:  Defined value of a given dimension for reference purposes

Units:  Defined value of a given dimension for reference purposes  Preferred system (in chemistry) is S.I.

Units:  Defined value of a given dimension for reference purposes  Preferred system (in chemistry) is S.I. DimensionS.I. Unit

Units:  Defined value of a given dimension for reference purposes  Preferred system (in chemistry) is S.I. DimensionS.I. Unit Mass kg

Units:  Defined value of a given dimension for reference purposes  Preferred system (in chemistry) is S.I. DimensionS.I. Unit Mass kg Length m

Units:  Defined value of a given dimension for reference purposes  Preferred system (in chemistry) is S.I. DimensionS.I. Unit Mass kg Length m Time s

Units:  Defined value of a given dimension for reference purposes  Preferred system (in chemistry) is S.I. DimensionS.I. Unit Mass kg Length m Time s Temperature K (kelvin)

Units:  Defined value of a given dimension for reference purposes  Preferred system (in chemistry) is S.I. DimensionS.I. Unit Mass kg Length m Time s Temperature K (kelvin) Amount of substance mol (mole)

Units:  Defined value of a given dimension for reference purposes  Preferred system (in chemistry) is S.I. DimensionS.I. Unit Mass kg Length m Time s Temperature K (kelvin) Amount of substance mol (mole) Current A (ampere)

Units:  Defined value of a given dimension for reference purposes  Preferred system (in chemistry) is S.I. DimensionS.I. Unit Mass kg Length m Time s Temperature K (kelvin) Amount of substance mol (mole) Current A (ampere) Luminous intensity cd (candela)

Common S.I. prefixes PrefixNameMeaning Ggiga10 9 Mmega10 6 kkilo10 3

Common S.I. prefixes PrefixNameMeaning Ggiga10 9 Mmega10 6 kkilo10 3 ddeci10 -1 ccenti10 -2 mmilli10 -3

Common S.I. prefixes PrefixNameMeaning Ggiga10 9 Mmega10 6 kkilo10 3 ddeci10 -1 ccenti10 -2 mmilli10 -3  micro10 -6 nnano10 -9 ppico10 -12

Derived Units Quantity Definition Derived Unit Area Length x length m 2

Derived Units Quantity Definition Derived Unit Area Length x length m 2 Volume Area x length m 3

Derived Units Quantity Definition Derived Unit Area Length x length m 2 Volume Area x length m 3 Density Mass/ unit volume kg m -3

Derived Units Quantity Definition Derived Unit Area Length x length m 2 Volume Area x length m 3 Density Mass/ unit volume kg m -3 Speed Distance/ unit time m s -1

Derived Units Quantity Definition Derived Unit Area Length x length m 2 Volume Area x length m 3 Density Mass/ unit volume kg m -3 Speed Distance/ unit time m s -1 Acceleration Change in speed/ m s -2 unit time

Derived Units Quantity Definition Derived Unit Area Length x length m 2 Volume Area x length m 3 Density Mass/ unit volume kg m -3 Speed Distance/ unit time m s -1 Acceleration Change in speed/ m s -2 unit time Force Mass x acceleration kg m s -2 (newton, N)

Derived Units Quantity Definition Derived Unit Area Length x length m 2 Volume Area x length m 3 Density Mass/ unit volume kg m -3 Speed Distance/ unit time m s -1 Acceleration Change in speed/ m s -2 unit time Force Mass x acceleration kg m s -2 (newton, N) Pressure Force/ unit area kg m -1 s -2 (pascal, Pa)

Derived Units Quantity Definition Derived Unit Area Length x length m 2 Volume Area x length m 3 Density Mass/ unit volume kg m -3 Speed Distance/ unit time m s -1 Acceleration Change in speed/ m s -2 unit time Force Mass x acceleration kg m s -2 (newton, N) Pressure Force/ unit area kg m -1 s -2 (pascal, Pa) Energy Force x distance kg m 2 s -2 (joule, J )

Difference between mass and amount of substance:  amount of substance is the number of specified entities (e.g. atoms, molecules, etc.)

Difference between mass and amount of substance:  amount of substance is the number of specified entities (e.g. atoms, molecules, etc.) EntityNumber of entitiesMass (g) Hg6.02 x 10 23 atoms200.59 (= 1 mol)

Difference between mass and amount of substance:  amount of substance is the number of specified entities (e.g. atoms, molecules, etc.) EntityNumber of entitiesMass (g) Hg6.02 x 10 23 atoms200.59 (= 1 mol) KCl6.02 x 10 23 molecules74.56 (= 1 mol)

Difference between mass and amount of substance:  amount of substance is the number of specified entities (e.g. atoms, molecules, etc.) EntityNumber of entitiesMass (g) Hg6.02 x 10 23 atoms200.59 (= 1 mol) KCl6.02 x 10 23 molecules74.56 (= 1 mol) SO 4 2- 6.02 x 10 23 ions96.06 (=1 mol)

Accuracy: measure of how close measurement is to its real value

Precision: measure of how close successive measurements are to each other

Accuracy: measure of how close measurement is to its real value Precision: measure of how close successive measurements are to each other X X X Precise & accurate

Accuracy: measure of how close measurement is to its real value Precision: measure of how close successive measurements are to each other X X X X X X Precise & accurate & inaccurate

Accuracy: measure of how close measurement is to its real value Precision: measure of how close successive measurements are to each other X X X X X X X X X Precise Precise Imprecise & accurate & inaccurate & inaccurate

Dimensional analysis: a method of reducing physical quantities to combinations of the 7 basic dimensions

Dimensional analysis: a method of reducing physical quantities to combinations of the 7 basic dimensions Q1. Dimensions of pressure?

Dimensional analysis: a method of reducing physical quantities to combinations of the 7 basic dimensions Q1. Dimensions of pressure? A. Pressure = Force/Area and we already know the dimensions of force are MLt -2. Thus the dimensions of pressure are MLt -2 /L 2 = ML -1 t -2.

Dimensional analysis: a method of reducing physical quantities to combinations of the 7 basic dimensions Q1. Dimensions of pressure? A. Pressure = Force/Area and we already know the dimensions of force are MLt -2. Thus the dimensions of pressure are MLt -2 /L 2 = ML -1 t -2. Q2. Check the validity of the following equation: PV = nR/T, given units of R to be ML 2 t -2 n -1 T -1.

Dimensional analysis: a method of reducing physical quantities to combinations of the 7 basic dimensions Q1. Dimensions of pressure? A. Pressure = Force/Area and we already know the dimensions of force are MLt -2. Thus the dimensions of pressure are MLt -2 /L 2 = ML -1 t -2. Q2. Check the validity of the following equation: PV = nR/T, given units of R to be ML 2 t -2 n -1 T -1. A. Dimensions of L.H.S.: ML -1 t -2. L 3 = ML 2 t -2 Dimensions of R.H.S.: n. ML 2 t -2 n -1 T -1 = ML 2 t -2 T -2

Dimensional analysis: a method of reducing physical quantities to combinations of the 7 basic dimensions Q1. Dimensions of pressure? A. Pressure = Force/Area and we already know the dimensions of force are MLt -2. Thus the dimensions of pressure are MLt -2 /L 2 = ML -1 t -2. Q2. Check the validity of the following equation: PV = nR/T, given units of R to be ML 2 t -2 n -1 T -1. A. Dimensions of L.H.S.: ML -1 t -2. L 3 = ML 2 t -2 Dimensions of R.H.S.: n. ML 2 t -2 n -1 T -1 = ML 2 t -2 T -2 Equating both sides does not cancel all terms, thus equation is invalid.

ATOMS AND MOLECULES

Atom:smallest particle of an element which can undergo chemical changes in a reaction

ATOMS AND MOLECULES Atom:smallest particle of an element which can undergo chemical changes in a reaction Molecule: smallest particle of a compound which can exist and still retain the chemical properties of the compound.

Structure of the Atom

Size:0.1 to 0.5 nanometers (1nm = 1x10 -9 m)

Structure of the Atom Size:0.1 to 0.5 nanometers (1nm = 1x10 -9 m) Mass:H atom = 1.67x10 -24 g = 1.008 atomic mass units (a.m.u.)

Structure of the Atom Size:0.1 to 0.5 nanometers (1nm = 1x10 -9 m) Mass:H atom = 1.67x10 -24 g = 1.008 atomic mass units (a.m.u.) C atom = 2x10 -23 g = 12.000 a.m.u.

Structure of the Atom Size:0.1 to 0.5 nanometers (1nm = 1x10 -9 m) Mass:H atom = 1.67x10 -24 g = 1.008 atomic mass units (a.m.u.) C atom = 2x10 -23 g = 12.000 a.m.u. Electrical charge: neutral

Structure of the Atom Size:0.1 to 0.5 nanometers (1nm = 1x10 -9 m) Mass:H atom = 1.67x10 -24 g = 1.008 atomic mass units (a.m.u.) C atom = 2x10 -23 g = 12.000 a.m.u. Electrical charge: neutral Composition: contains electrons, protons, and, with the exception of hydrogen, neutrons.

Structure of the Atom Size:0.1 to 0.5 nanometers (1nm = 1x10 -9 m) Mass:H atom = 1.67x10 -24 g = 1.008 atomic mass units (a.m.u.) C atom = 2x10 -23 g = 12.000 a.m.u. Electrical charge: neutral Composition: contains electrons, protons, and, with the exception of hydrogen, neutrons. ParticleMass (a.m.u.)Charge e- 0.0005 -1

Structure of the Atom Size:0.1 to 0.5 nanometers (1nm = 1x10 -9 m) Mass:H atom = 1.67x10 -24 g = 1.008 atomic mass units (a.m.u.) C atom = 2x10 -23 g = 12.000 a.m.u. Electrical charge: neutral Composition: contains electrons, protons, and, with the exception of hydrogen, neutrons. ParticleMass (a.m.u.)Charge e- 0.0005 -1 p+ 1.007 +1

Structure of the Atom Size:0.1 to 0.5 nanometers (1nm = 1x10 -9 m) Mass:H atom = 1.67x10 -24 g = 1.008 atomic mass units (a.m.u.) C atom = 2x10 -23 g = 12.000 a.m.u. Electrical charge: neutral Composition: contains electrons, protons, and, with the exception of hydrogen, neutrons. ParticleMass (a.m.u.)Charge e- 0.0005 -1 p+ 1.007 +1 n 1.009 0

Structure of the Atom

Size:0.1 to 0.5 nanometers (1 nm = 1 x 10 -9 m)

Structure of the Atom Size:0.1 to 0.5 nanometers (1 nm = 1 x 10 -9 m) Electron clouds ~ 2 x 10 -10 m

Structure of the Atom Size:0.1 to 0.5 nanometers (1 nm = 1 x 10 -9 m) Nucleus Electron clouds ~ 2 x 10 -10 m

Structure of the Atom Size:0.1 to 0.5 nanometers (1 nm = 1 x 10 -9 m) Nucleus Electron clouds ~ 5 x 10 -15 m ~ 2 x 10 -10 m

Structure of the Atom Size:0.1 to 0.5 nanometers (1 nm = 1 x 10 -9 m) Nucleus Electron clouds ~ 5 x 10 -15 m ~ 2 x 10 -10 m Nucleus- consists of protons and neutrons

“Life-sized” model of the atom

“Scaled up” electron mass Electron = 0.0005 a.m.u.Proton = 1.0070 a.m.u.

“Life-sized” model of the atom “Scaled up” electron mass Electron = 0.0005 a.m.u.Proton = 1.0070 a.m.u. “Model proton” = 65 kg“Model electron” = 32 g

“Life-sized” model of the atom “Scaled up” electron mass Electron = 0.0005 a.m.u.Proton = 1.0070 a.m.u. “Model proton” = 65 kg“Model electron” = 32 g “Scaled up” atomic radius Nuclear diameter = 5 x 10 -15 m Atomic diameter = 2 x 10 -10 m

“Life-sized” model of the atom “Scaled up” electron mass Electron = 0.0005 a.m.u.Proton = 1.0070 a.m.u. “Model proton” = 65 kg“Model electron” = 32 g “Scaled up” atomic radius Nuclear diameter = 5 x 10 -15 m Atomic diameter = 2 x 10 -10 m “Model nucleus” radius = 1 m “Model atomic” radius = 40 km

“Life-sized” model of the atom “Scaled up” electron mass Electron = 0.0005 a.m.u.Proton = 1.0070 a.m.u. “Model proton” = 65 kg“Model electron” = 32 g “Scaled up” atomic radius Nuclear diameter = 5 x 10 -15 m Atomic diameter = 2 x 10 -10 m “Model nucleus” radius = 1 m “Model atomic” radius = 40 km Q. A speck of carbon contains ca. 10 19 atoms and the diameter of a carbon atom is 1.5 x 10 -10 m. If the circumference of the earth is 40,075 km, how many times around the earth would a line of single carbon atoms extend?

“Life-sized” model of the atom “Scaled up” electron mass Electron = 0.0005 a.m.u.Proton = 1.0070 a.m.u. “Model proton” = 65 kg“Model electron” = 32 g “Scaled up” atomic radius Nuclear diameter = 5 x 10 -15 m Atomic diameter = 2 x 10 -10 m “Model nucleus” radius = 1 m “Model atomic” radius = 40 km Q. A speck of carbon contains ca. 10 19 atoms and the diameter of a carbon atom is 1.5 x 10 -10 m. If the circumference of the earth is 40,075 km, how many times around the earth would a line of single carbon atoms extend? A. Length = 10 19 x 1.5 x 10 -10 m = 1.5 x 10 9 m. # times = 1.5 x 10 9 /40075 x 10 3 = 37.4

Iron atoms on a copper crystal

Iron atoms on a copper crystal Carbon monoxide molecules on platinum crystal

Iron atoms on a copper crystal Xenon atoms on nickel Carbon monoxide molecules on platinum crystal

Atomic number:number of protons in an atom. Symbol: Z Atomic mass: mass of an atom in a.m.u. (  number of protons + neutrons in an atom). Symbol: A

Atomic number:number of protons in an atom. Symbol: Z Atomic mass: mass of an atom in a.m.u. (  number of protons + neutrons in an atom). Symbol: A Atome-p+nZA (a.m.u.) H11011.008 Li33437.016 C666612.000 U929214692238.05

Conventional Notation for Chemical Symbols Cl

Conventional Notation for Chemical Symbols Cl 35 17 - 2 Mass numberNumber and sign of charge

Conventional Notation for Chemical Symbols Cl 35 17 - 2 Mass numberNumber and sign of charge Atomic number Number of atoms in entity

Conventional Notation for Chemical Symbols Cl 35 17 - 2 Mass numberNumber and sign of charge Atomic number Number of atoms in entity Examples: He 4 2 OH - CO 3 2-

Ions:atoms or molecules which have gained or lost one or more electrons Isotopes: atoms of the same element which have different masses, i.e. different numbers of neutrons

Ions:atoms or molecules which have gained or lost one or more electrons Isotopes: atoms of the same element which have different masses, i.e. different numbers of neutrons Examples of ions:H + H - NO 3 -

Ions:atoms or molecules which have gained or lost one or more electrons Isotopes: atoms of the same element which have different masses, i.e. different numbers of neutrons Examples of ions:H + H - NO 3 - Examples of isotopes:H 1 1 H 1 2 H 3 1 Hydrogen Deuterium Tritium

ElementsCompounds AtomsMolecules Identical atoms

ElementsCompounds AtomsMolecules IonsIsotopes Identical atoms ± e - ± n

ElementsCompounds AtomsMolecules IonsIsotopes Identical atoms ± e - ± n ± e - ± n

Test Tubes General Chemistry A CH4701. This lecture:  General information  Course syllabus  Recommended texts  Relevance of this module to you.

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Test Tubes General Chemistry A CH4701. This lecture:  General information  Course syllabus  Recommended texts  Relevance of this module to you.

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