Lecture outline: Chapter 2 ~400 B C400 B.C. 1. Atomic ...ion.chem.usu.edu/~ensigns/chem1210/lectureoverheads...1. Atomic structure 2. The Periodic Table 3. Molecules and ions 4. Naming

Lecture outline: Chapter 21. Atomic structure2. The Periodic Table3. Molecules and ions4 Naming ionic and molecular compounds4. Naming ionic and molecular compounds

S. Ensign, Atomic structure & nomenclature1

~400 B C400 B.C.

Can matter be divided endlessly into smaller and smaller pieces or and smaller pieces, or is there a point at is there a point at which it can’t be


divided anymore??

The Atomic Theory of Matter• John Dalton:

Each element is composed of atoms–Each element is composed of atoms–All atoms of an element are identical.–In chemical reactions, the atoms are

not changed Pb + Snot changed.–Compounds are formed when atoms

f th l t bi

Pb + S

of more than one element combine.


Dalton’s law of multiple proportionsAtoms join together in small whole number ratios to make compoundsnumber ratios to make compounds

OHH

C OO H NH

CH

HH CH

HH OO C OO H NH

CH

HH CH

HH O

Atoms can combine in different ratios to make different compoundsratios to make different compounds

OHH

O HH O H NH

NH

NH


O O HH O H NH

NH

NH

Atoms of element 1

Atoms of l t 2

Compounds of l t 1 d 2

Mixture of l t 1 d 2element 1 element 2 elements 1 and 2 elements 1 and 2

OH

OH O

HHO

H HO O

O

HH

H

O OH H

O

O HOO

HH

H H

O

OH

HH

OHH


Observations/studies of two phenomena were key to determiningphenomena were key to determining

the structure of the atom • Electricity

Separable charges are associated with matter

• RadioactivitySeparable charges are associated with matter

y

Atoms are composed of subatomic particles


Atoms are composed of subatomic particles

Three types of radiation emitted from radioactive uraniumradioactive uranium

(-) α particle+2(-)

(+)γ ray

(+) β particleUranium source

-1

Electrically h d Detector


charged plates

Detector

Fun household sources of radioactivityFi t ( i k 1970 d li ) th• Fiestaware (cirka 1970 and earlier): the orange color comes from uranium salts

• Lantern mantles (Thorium)


• Smoke detectors (Americium)

Atomic Structure: components of the atom

electrons Charge: -1.60 x 10-19 C “(-1)”Mass: 9.109 x 10-28 g

protons: found in the nucleus, they have a positive charge equal in magnitude to thepositive charge equal in magnitude to the electron’s negative charge.

Charge: +1 60 x 10-19 C “(+1)”

neutrons: found in the nucleus virtually

Charge: +1.60 x 10 C (+1)Mass: 1.673 x 10-24 g

neutrons: found in the nucleus, virtually same mass as a proton but no charge.

Charge: neutral


gMass: 1.675 x 10-24 g

Atomic structureWhat are the subatomic particles how big• What are the subatomic particles, how big are they, and how massive are they?

• How do the subatomic particles associate in atoms?

• Plum pudding model: (incorrect)


The Rutherford experiment

+2+2+2+2+2+2+2+2+2+2+2+2+2+2+2+2+2+2+2

Alpha particle source Thin gold sheet


Detector

Interpretation of Rutherford’s of Rutherford s experiment


The atom is mostly empty space, with the majority of the mass concentrated in a small, dense region

Nucleus (proton(s) and neutron(s)~10-18 cm

electron: “orbits” the nucleuselectron: orbits the nucleus

“multielectron atoms” have more than one e- “orbiting” the nucleus

10 13


~10-13 cm

Diameter of atom ~ 10-8 cm (~1-5 Å)

The electron is ~1000 times smaller in size than the proton, but occupies a space ~10,000-100,000 times

greater than the size of the nucleus

Golf ball nucleus on 50 yard line(2 cm diameter)

The stadium ( 200 m diameter) represents the space in which the electron(s) reside!


electron(s) reside!

How small is an atom???

Density of a nucleus?Density of a nucleus?Nucleus (proton(s) and neutron(s)

p+

p+np+

n

electron: “orbits” the nucleus

p

n

p+p+

n


Like forces repel, opposites attract, so…

What holds the nucleus together?

Why don’t the electrons fall into the nucleus??nucleus??

Nucleus (proton(s) and neutron(s)Nucleus (proton(s) and neutron(s)

p+nn

electron: “orbits” the nucleus


p+

n

p+n

p+n

Four basic attractive forces in natureFour basic attractive forces in nature

• Gravitational (masses)

Ma Gravitational (masses)

• Electromagnetic (electrically charged and/or magnetized)

agnitude o and/or magnetized)• Weak nuclear force

S f

of force inc

• Strong nuclear force

creases

p+

p+np+

n

p+n


nn

What defines the atoms of a What f n s th atoms of a single element?

If all atoms consists of protons, neutrons, and electrons, then what makes oxygen oxygen and carbon carbon?


Elements are classified on the basis of the number of protons in the nucleusnucleus

All t f i l t h thAll atoms of a given element have the same number of protons in the nucleus

Z= atomic number = # of protons in pthe nucleus


Elements are classified on the basis of the number of protons in the nucleus

All atoms of a given element have the same number of protons in the nucleus

f p

Z= atomic number = # of protons in the nucleus


How many neutrons and electrons i i ?in a given atom?

• # e- = # p+# e = # p• # neutrons can vary

(# + # ) #• Σ (# p+ + # n) = mass #


Atomic Symbols

X ← Element SymbolAMass number →

X ← Element Symbol

ZAtomic number →

39 K ← Element Symbol39Mass number →

K y

19Atomic number →


Isotopes: atoms of an element that differ in the number of neutrons in thediffer in the number of neutrons in the nucleus

Isotopes have the same atomic pnumber but different mass numbers


Two isotopes of carbon

p+

p+ nn p+

np+

p+p+nn

Carbon-12p+

p+ nn p+

np+

p+p+nn

Carbon-13n

n p+p+ n p+p+

6 protons6 neutrons

6 protons7 neutrons7 neutrons

12 136

12C 613C


Hydrogen, the simplest element


Silver has two isotopes: one with 60 ne trons one ith 62 ne trons Whatneutrons, one with 62 neutrons. What are the mass numbers and symbols of these isotopes?

For silver (Ag), Z = 47( g),


Give the complete symbol for each of the following atoms

ZAX

for each of the following atoms

Sodium with 12 neutronsSodium with 12 neutrons

argon with 21 neutronsFor Na, Z = 11

argon with 21 neutrons

Gallium with 39 neutronsFor Ar, Z = 18

Gallium with 39 neutronsFor Ga, Z = 31


How many e- p+ and n are present inHow many e , p and n are present in an atom of:

40Ca See the Periodic

119SnTable to find the atomic numbers for

244Pthese elements

244Pu


Complete the following table using the Periodic Table and the information provided

Symbol 46Ti 127TeSymbol Ti Te

# protons 45

# neutrons 58 18

Atomic # 16 38

Mass # 88


What is the origin of the name of the “uncola” beverage “7 up”?uncola beverage 7 up ?


Atomic weights: We will cover this material in lecture 7material in lecture 7


The Periodic Table


The Periodic Table


The Periodic TableHorizontal rows = “periods” n = 1,2,3,4,5,6,7

n = 1

n = 2n = 3

n = 4n = 5n 5n = 6

n = 7n = 7

n = 6


n = 7

The Periodic Tablevertical columns = “families” or “groups”vertical columns families or groups

n = 1

n = 2n = 3

n = 4n = 5n 5n = 6

n = 7n = 7

n = 6


n = 7

The Periodic TableMetals, metalloids, and nonmetals


The Periodic TableSome important group names

Alka

met

Alka

met

hal

Nob

gaslials

aline earthtals

ogens

ble ses

The transition metals


Elements within groups (families) have similar chemical propertiessimilar chemical properties


Elements within groups (families) have similar chemical propertiessimilar chemical properties

Chemical properties of alkali metals:• react vigorously with water to produce hydrogen gas•React vigorously with oxygen to produce metal hydroxides•React vigorously with oxygen to produce metal hydroxides•React vigorously with halogens to produce saltsPhysical properties of alkali metals:•Soft metal•Silver-colored•Low density•Low melting and boiling points


Elements Essential for LifeElements Essential for Life


Molecular and ionic compoundsMolecular and ionic compounds•114 elements by themselves = ~114 substances (yawn)

•“Glue” different elements together in gdifferent ratios infinite number of potentially interesting compounds!!


A molecule (molecular compound; covalent compound)covalent compound)

An assembly of two or more nonmetalyatoms, tightly bound (bonded) together

•Molecules of a single atom

•Molecules of more than one type of atomyp


Chemical formulas for molecules•Molecular formula: the actual numbers of•Molecular formula: the actual numbers of atoms of each element in the compound

•Empirical formula: the simplest whole number ratio of elements in the compoundp


Some compounds cannot be represented by a “molecular” formula

“Allotropes” of carbon: diamond, graphite, and buckyballp g p y

S. Ensign, Atomic structure & nomenclature44Graphite, Cn diamond, Cn buckyball, C60

Structural formulaA pictorial representation of a molecular formula Shows how the molecular formula. Shows how the atoms are joined together.


Molecular formula: the numbers of atoms of each element in the molecule

NH3

Structural formula: A pictorial representation showing how atoms are connected (arranged) inshowing how atoms are connected (arranged) in the compound

P ti d i A t t l f l idiPerspective drawing: A structural formula providing information about the 3-dimensional shape of the molecule

Ball and stick model: A perspective drawing where bonded atoms are shown as balls and sticksbonded atoms are shown as balls and sticks

Space filling model: A 3-dimensional model showing the relative sizes of individual atoms and


showing the relative sizes of individual atoms and their distances from one another

Subscripts and superscriptsSubscripts and superscripts• For an element, subscripts and superscripts to the

LEFT of the element indicate the atomic numberLEFT of the element indicate the atomic number and mass number of that element P32

15• For a compound subscripts to the RIGHT of the

P15• For a compound, subscripts to the RIGHT of the

elements tell us how many atoms of that element are present in the compound (no subscript = 1)p p ( p )– CH4, C2H4, CO2, H2O, NH3


Ions: atoms that have gained orIons: atoms that have gained or lost electrons and hence have a net

ti iti h Thnegative or positive charge. The nucleus of the atom remains unchanged.

C ti l t ( ) d Xn+• Cations: electron(s) removed Xn+

• Anions: electron(s) added Yn-


Formation of a sodium cation

11 11 p+

Remove one e-

11 p+ 11 p+

11 p+

11 e-

11 p+

10 e-11 e 10 e

Na Na1+ = Na+


Formation of a chloride anion

17

add one e-

1717 p+ 17 p+

17 p+

17 e-17 p+

18 e-17 e

Cl18 e

Cl-


IonsIons

• Metal atoms lose electrons to form cationsMetal atoms lose electrons to form cations• Nonmetal atoms gain electrons to make

anionsanions• WHY??


Many atoms gain or lose electrons in order to obtain the same number of electrons as a nearby noble gassame number of electrons as a nearby noble gas

Li+ F-N3-

H+ H-

O2-

Na+

K+

Cl-

B

N

P3-

O

S2-

S2

Mg2+

C 2+

Al3+

K+

Rb+

Br-

I-

S2-

Te2-

Ca2+

Sr2+

Cs+ Ba2+


Predict the charges on the ions formed by the following y gelements:

Element nearest noble gas ionNaMgCsRaRaFClONP


PAlC

Complete the following table using the Periodic Table and the information provided

Symbol 85Y 120Sn2+ 127Te

# protons 65

# neutrons 94 32

# electrons 63 27

Atomic # 53

Mass # 127

Charge 0 -1


Binary ionic compoundsy pCombinations of metal cations and nonmetal anions bonded togethernonmetal anions bonded together through strong electrostatic attractive forces (an “ionic bond”)forces (an ionic bond )

Contrast molecular compounds, which areContrast molecular compounds, which are formed from combinations of nonmetals only (H2O, CO2, CH4, etc.) bonded by shared(H2O, CO2, CH4, etc.) bonded by shared electron pairs in a “covalent bond”Combinations of metalloids and nonmetals


S. Ensign, Chem. 121055

Combinations of metalloids and nonmetals are usually classified as “molecular”

Reaction of Na and Cl

Ionic compounds are always represented by empirical formulas: there is no discrete molecular formula for an ionic


formulas: there is no discrete molecular formula for an ionic solid

Writing empirical formulas for ionic compoundsA d i h l 2 l i “bi• A compound with only 2 elements is a “binary compound”F i i d l th b l f th• For ionic compounds, place the symbol for the metal before that of the nonmetal (cation first, anion second)anion second)

• Subscripts after the elements designate the number of atoms of that type in the compoundnumber of atoms of that type in the compound

• When writing the formula of a neutral ionic compound, net charge = 0, so the charges mustcompound, net charge 0, so the charges must balance for each ion


Writing empirical formulas for ionic compounds• A compound with only 2 elements is a “binary• A compound with only 2 elements is a binary

compound”• For ionic compounds, place the symbol for the metal

before that of the nonmetal (cation first, anion second))

• Subscripts after the elements designate the number of atoms of that type in the compound

• When writing the formula of a neutral ionic compound, net charge = 0, so the charges must balance for each ion


Writing empirical formulas for ionic compounds• A compound with only 2 elements is a “binary• A compound with only 2 elements is a binary

compound”• For ionic compounds, place the symbol for the metal

before that of the nonmetal (cation first, anion second))

• Subscripts after the elements designate the number of atoms of that type in the compound

• When writing the formula of a neutral ionic compound, net charge = 0, so the charges must balance for each ion


Polyatomic ions: a compound of two or more nonmetal atoms joined throughmore nonmetal atoms, joined through covalent bonds, that forms a single charged unit (i e a molecular compoundcharged unit (i.e., a molecular compound that does not have a neutral charge)

SO3 is a molecular compoundSO4

2- is a polyatomic anion

NH3 is a molecular compoundNH4

+ is a polyatomic cation4 p y


Common polyatomic ionsCommon polyatomic ionsName Formula Charge

A i i NH + +1Ammonium ion NH4+ +1

Nitrate ion NO3- -1

Chlorate ion ClO3- -1

Carbonate ion CO32- -2Carbonate ion CO3 2

Sulfate ion SO42- -2

Peroxide ion O22- -2

Phosphate ion PO43- -3


Ionic compounds containing polyatomic ionsName Formula Charge

Ammonium ion NH4+ +1XmYn Nitrate ion NO3- -1


Carbonate ion CO 2- 2

XmYn

Carbonate ion CO32- -2


Peroxide ion O22- -2Peroxide ion O2 2



A fail proof way to write the correct formula for an ionic compoundfor an ionic compound

Xn+ Ym-Xn Ymnm

X YXmYn

R d t i i l f l if b di idi b th


Reduce to an empirical formula, if necessary, by dividing by the appropriate integer (e.g. Mg2O2 MgO)

A fail proof way to deduce the ion charges on ions present in an ionic compound

X Yon ions present in an ionic compound

n+ m-XmYn

Xn+ Ym-

Be sure the magnitude of the ion charge matches what it should


g gbe based on position in the periodic table for a monatomic ion, or the known charge for a polyatomic ion

Write empirical formulas for the bi i i d f d f binary ionic compounds formed from the combinations of Co2+, Mg2+, and Li+ with S2-, PO4

3-, and SO42-


Classify the following compounds as ionic or molecular. Which molecular formulas are also empirical formulas?p

compound Type? Empirical?NF33

C6H14

K2SP SP4S3

MgOKBrOF2

AsH3

XeF2

NaFPbF2


2

P2F4

Nomenclature: The naming of substancesB bl tBe able to name:•Constituent atoms in molecular compoundsC tit t i i i i d•Constituent ions in ionic compounds

•Ionic compoundsM l l d

I i d d i diff t

•Molecular compounds•AcidsIonic compounds are named using a different set of rules than covalent compounds


Naming ionic compoundsNaming ionic compounds

• Cation name followed by anion nameCation name followed by anion name• So, how do we name cations and anions?


Naming monatomic cations (+ ions)• Cations for which only one charge can be formed

(group 1A, 2A, 3A, some “d” block): the name is simply the name of the metal followed by “ion”simply the name of the metal followed by “ion”

• Cations of transition (“d block”) metals that can form more than one charge:form more than one charge:– “New” method: Place the charge in parentheses after the

metal name and before “ion”– “old” method for metals that form two charges: use root

of latin name + “ous” for lower charge, or “ic” for higher h f ll d b “i ”charge, followed by “ion”


Naming monatomic cations (+ ions)Cations for which only one charge can be formed

(group 1A 2A 3A some “d” block): the name(group 1A, 2A, 3A, some d block): the name is simply the name of the metal followed by “ion”


Naming monatomic cations (+ ions)Cations of transition metals that can form more

than one charge:than one charge:“New” method: Place the charge in

parentheses after the metal name and before “ion”

“old” method for metals that form twoold method for metals that form two charges: use root of latin name + “ous” for lower charge, or “ic” for higher charge, followed by “ion”


There aren’t many polyatomic cations to worry aboutCommon polyatomic ionsCommon polyatomic ionsName Formula Charge

A i i NH + +1Ammonium ion NH4+ +1

Nitrate ion NO3- -1


Carbonate ion CO32- -2Carbonate ion CO3 2


Peroxide ion O22- -2



Naming monatomic anions (- ions)• Drop the ending of the name of the elementDrop the ending of the name of the element

and add “ide” + “ion”H-HN3-

O2-O2

F-

S2S2-

Br-


There are a lot more polyatomic anions to worry about


Making sense of polyatomic anion namesMaking sense of polyatomic anion names

• Some of them also end in “ide”Some of them also end in ide– Hydroxide (know this one now)

Cyanide– Cyanide– Peroxide

azide– azide


Making sense of polyatomic anion namesXO m• Oxyanions are very common

– Elements that form only 2 oxyanions:XOn

m-

• Charges on both ions are generally the same• One with less oxygens = “ite”

O ith “ t ”• One with more oxygens = “ate”– Elements that form 3 or 4 oxyanions:

Ch b th i ll th• Charges on both ions are generally the same• hypo = less• per = moreper = more

– Hydrogen ions (H+) can combine with oxyanions to form “new” hydrogen oxyanions


oxyanions to form new hydrogen oxyanions

Making sense of polyatomic anion namesXO m

• Note I am going to give you the formulas XOn

m-

g g g yand names for the following oxyanions on the exam information sheet. At some point pyou will need to memorize these though.

Formulas and names of common polyatomic ions:

Carbonate ion = CO32- Sulfate ion = SO4

2-3 4

Nitrate ion = NO3- Perchlorate ion = ClO4

-

Ph h t i PO 3


Phosphate ion = PO43-

Making sense of polyatomic anion namesXOXOn

m-• Elements that form only 2 oxyanions:

• Charges on both ions are generally the same• Charges on both ions are generally the same• One with less oxygens = “ite”• One with more oxygens = “ate”

Formulas and names of common polyatomic ions:Carbonate ion = CO3

2- Sulfate ion = SO42-


-

Phosphate ion = PO43-yg

• Nitrogen combines with O to form two common oxyanions that have one N: NO2

- and NO3-oxyanions that have one N: NO2 and NO3

• Since we know from the table that NO3- is the

nitrate ion, we can predict that NO2- is the nitrite ionnitrate ion, we can predict that NO2 is the nitrite ion

• Note the ion charges on NO2- and NO3

- are the same (-1 in each case)


( )


m-• Elements that form only 2 oxyanions:

• Charges on both ions are generally the same• Charges on both ions are generally the same• One with less oxygens = “ite”• One with more oxygens = “ate”




-


• Sulfur combines with O to form two common oxyanions that have one S: SO3

2- and SO42-oxyanions that have one S: SO3 and SO4

• Since we know from the table that SO42- is the

sulfate ion, we can predict that SO32- is the sulfitesulfate ion, we can predict that SO3 is the sulfite

ion• Note the ion charges on SO3

2- and SO42- are the


g 3 4same (-2 in each case)

Making sense of polyatomic anion namesXO• Elements that form only 2 oxyanions:

• Charges on both ions are generally the same

XOnm-

• Charges on both ions are generally the same• One with less oxygens = “ite”• One with more oxygens = “ate”




-


• Phosphorus combines with O to form two common oxyanions: PO3

3- and PO43-common oxyanions: PO3 and PO4

• Since we know from the table that PO43- is the

phosphate ion, we can predict that PO33- is thephosphate ion, we can predict that PO3 is the

phosphite ion• Note the ion charges on PO3

3- and PO43- are the g 3 4

same (-3 in each case)S. Ensign, Atomic structure & nomenclature

80


m-

• Carbon combines with O to form only common oxyanion with one C: CO3

2-

• CO32- is the carbonate ion, and there is no such

thing as the carbonite ionFormulas and names of common polyatomic ions:Carbonate ion = CO3



-



Making sense of polyatomic anion names• Elements that form 4 oxyanions: XOn

- , where “X” is a halogen (Cl, Br, I) and n = 1-4 Formulas and names of common polyatomic ions:

Carbonate ion = CO32- Sulfate ion = SO4

2-


-


• Charges on all 4 ions are the same (-1)• Take the root of the halogen (chlor, bromo, g ( , ,

iodo)• Hypo___ ite = XO- (e.g. hypochlorite)• ___ ite = XO2

- (e.g. chlorite)• ate = XO2

- (e.g. chlorate)


___ 2 ( g )• Per ___ ate = XO4

- (e.g. perchlorate)

Oxyanions can also be formed with the formulas X O p- and have names that areformulas XnOm

p and have names that are not easy to predict. You do not need to memorize or be familiar with any of thesememorize or be familiar with any of these for chemistry 1210

• S2O32- is the thiosulfate ion

S O 2 i th dithi t i• S2O42- is the dithionate ion

• S4O62- is the tetrathionate ion


There are a few oxyanions consisting of metals combined with oxygens bondedmetals combined with oxygens, bonded similarly to the bonds between nonmetals and oxygens in oxyanions You don’t needand oxygens in oxyanions. You don t need to memorize the names of these now, but h lhere are a couple common ones.

• MnO4- = permanganate ion (used widely in gen

chem labs)• Cr2O7

2- = dichromate ion (also used widely in gen chem labs)


Oxyanion examples– Elements that form only 2 oxyanions:

XOnm-

• Charges on both ions are generally the same• One with less oxygens = “ite”• One with more oxygens = “ate”

– Elements that form 3 or 4 oxyanions:Elements that form 3 or 4 oxyanions:• Charges still the same• hypo = less• per = more

H d i (H+) bi ith i t– Hydrogen ions (H+) can combine with oxyanions to form “new” hydrogen oxyanions


Information I will give you on examInformation I will give you on examFormulas and names of common polyatomic ions:

C b t i CO 2-Carbonate ion = CO32

Nitrate ion = NO3-


2Sulfate ion = SO42-

Perchlorate ion = ClO4-

Ammonium ion = NH4+Ammonium ion NH4

You must know the hydroxide ion (OH-)You must know the hydroxide ion (OH )


Naming ionic compounds:C ti f ll d b i•Cation name followed by anion name

•Examples: Name the following ionic compounds:Formulas and names of common polyatomic ions:

2

•CaBr2

•Mg(OH)2

Carbonate ion = CO32-

Nitrate ion = NO3-


Sulfate ion = SO42-

Perchlorate ion = ClO4-

Ammonium ion = NH +Mg(OH)2

•Co2O3

Ammonium ion = NH4

•TiCl2

•(NH4)2CO3( 4)2 3

•Na2SO4Wherever possible, predict charges on simple cations and anions based on


•NaHSO4and anions based on positions in periodic table

Acids• A simple working definition (for now): a

compound that dissolves in water to produce p phydrogen ions and a corresponding anion

HnX


Naming acids HnX• Binary acids:

– Begin with “hydro”

n

eg yd o– Follow “hydro” with anion name, replacing “ide”

with “ic”– Complete the naming with “acid”


Adding hydrogens to oxyanions to form neutral acids:

mH+ + XOnm- HmXOn

• Change “___ite ion” to “___ous acid• Change “ ate ion” to ous acidChange ___ate ion to ___ous acid• Retain “hypo” or “per” if they are present


Oxyanion ion Formula Oxyacid Formula

Nitrite ion NO2- Nitrous acid HNO2

Nitrate ion NO3- Nitric acid HNO3

Hypochlorite ion ClO3- Hypochlorous acid HClO

chlorite ion ClO2- Chlorous acid HClO2

chlorate ion ClO3- Chloric acid HClO3

Perchlorate ion ClO4- Perchloric acid HClO4

Carbonate ion CO32- Carbonic acid H2CO3Carbonate ion CO3 Carbonic acid H2CO3

Sulfate ion SO32- Sulfurous acid H2SO3

Sulfate ion SO42- Sulfuric acid H2SO4

Phosphite ion PO33- Phosphorous acid H3PO3

Phosphate ion PO43- Phosphoric acid H3PO4


Naming molecular compoundsNaming molecular compounds

• Nonmetal + nonmetalNonmetal + nonmetal• Many are “binary”


Naming binary molecular compounds:In general the element closer to the metals is listed first•In general, the element closer to the metals is listed first

•the first element in the formula is named first, using it’s normal elemental name

•For the second element in the formula , drop the ending of the element name and replace with “ide”

•Use prefixes to indicate the number(s) of atom(s) in theUse prefixes to indicate the number(s) of atom(s) in the binary compounds (don’t use “mono” for 1st element)

-Mono-Di-Tri-Tetra


-penta

Prefixes used when naming binary molecular compoundsPrefix Meaningmono 1di 2di 2tri 3tetra 4tetra 4penta 5hexa 6hepta 7nona 8deca 9


Naming binary molecular compounds:•In general, the element closer to the metals is listed first

•the first element in the formula is named first, using it’s normal elemental name

•For the second element in the formula , drop the ending of the element name and replace with “ide”

•Use prefixes to indicate the number(s) of atom(s) in the binary compounds (don’t useatom(s) in the binary compounds (don t use “mono” for 1st element)


Name these molecular and ionic compoundscompound Type? Empirical? NameNF3

C6H14C6H14

K2SP4S3

MgOKBrOFOF2

AsH3

XeF2

NaFPbF2

P F


P2F4

Give formulas for each of the following ionic compoundsmp

a) Ammonium nitrateb) Cobalt (II) nitrateb) Cobalt (II) nitratec) Nickel (II) sulfated) Ni k l (III) idd) Nickel (III) cyanidee) Vanadium (III) oxidef) Ammonium sulfate

Formulas and names of common polyatomic ions:

Carbonate ion = CO32-

Nitrate ion = NO3-



Phosphate ion = PO4 Sulfate ion = SO4

2- Perchlorate ion = ClO4

- Ammonium ion = NH4

+

Name the following compounds:

a) MgBr2

b) Li COb) Li2CO3

c) KHSO3

d) KMnO4

e) (NH4)2Se) (NH4)2Sf) CuClg) CuClg) CuCl2


Give formulas for:

a) Carbon dioxideb) Phosphor s triiodideb) Phosphorus triiodidec) Sulfur dichlorided) Xenon trioxidee) Dioxygen difluoridee) Dioxygen difluoride


Name the following molecular compounds:

a) N2F4

b) HBrb) HBrc) SF4

d) ClF3

e) BCl3e) BCl3f) P4O10


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Lecture outline: Chapter 2 ~400 B C400 B.C. 1. Atomic ...ion.chem.usu.edu/~ensigns/chem1210/lectureoverheads...1. Atomic structure 2. The Periodic Table 3. Molecules and ions 4. Naming