ionic compounds notes with added notes from …...ionic compounds notes with added notes from...

Ionic Compounds Notes with added notes from class.notebook November 08, 2016

Ionic Compoundsand

Ionic Bonding

Table of Contents: Ionic Compounds and Ionic BondingClick on the topic to go to that section

• Periodic Table Review

• Valence Electrons and the Octet Rule• Ions• Ionic Bonding

• Predicting an Ionic Compound's Formula

• Naming Ionic Compounds

• Properties of Ionic Compounds

• Formulas and Names of Ionic Compounds with Transition Metals

• Polyatomic ions• Formula and Names of Compounds with Polyatomic ions (Ternary Ionic Compounds)

• Polyatomic Patterns

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Periodic Table Review

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Periodic Table Review

The periodic table is "periodic" because of certain trends that are seen in the elements.

Some of these trends are atomic size, ionization energy, electronegativity and metallic character.

Elements from the same family/group have similar chemical properties because of their similar electron configuration.


The Periodic Table of the Elements

As

BSi

TeGe

Sb?

The periodic table can be divided into three large classifications of elements.

What type of elements are highlighted in blue, in yellow and in pink? What is unique about the elements that are highlighted in pink?

As

BSi

TeGe

Sb?

More metallic Less metallic Nonmetallic

Most metallic

Metallic Character of the ElementsWhen comparing elements in a period (row) , elements on the left generally have a "weaker" pull on their electrons due to the fewer protons in the nucleus.

The weaker the pull on electrons, the more easily the electrons are lost, and the greater the metallic character of the element.


As

BSi

TeGe

Sb?

More metallic Less metallic Nonmetallic

Most metallic

Metallic Character of the ElementsAs one moves down a column in the periodic table, atoms become larger due to more filled orbitals. The larger the atom, the farther the outer electrons are from the nucleus, and the easier it is for the atom to lose those electrons.

The easier it is to lose electrons, the more metallic the element.

1 Elements __________ exhibit similar physical and chemical properties.

A with similar chemical symbolsB with similar atomic masses

C in the same period of the periodic table

D on opposite sides of the periodic table

E in the same group of the periodic table

Answer


2 Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?

A Li, NaB Cs, BaC Ca, SiD Ga, GeE C, O

Answer

3 Which of the following is a nonmetal?

A WB SrC OsD IrE S

Answer


4 Potassium is a __________ and chlorine is a __________.

A metal, nonmetalB metal, metalC metal, metalloidD metalloid, nonmetalE nonmetal, metal A

nswer

#. Which element from each pair is more metallic?

Sodium or Sulfur?

Calcium or Francium?

Magnesium or Fluorine?


Valence Electrons and the Octet Rule


Octet Rule: Atoms will gain, lose, or share electrons in order to have complete outer shells of electrons (This gives the atom stability).

A full outer shell in most atoms will contain 8 electrons:2 electrons in the s subshell and6 electrons in the p subshell ( s2p6 configuration)

Small atoms, like Li, Be, and B, will lose electrons to have a full s2 configuration. This is called a duet.

Octet Rule

Which elements on the periodic table have a complete outer shell? What is true about these elements relative chemical reactivity?


Valence Electrons

Valence electrons are the electrons in the highest occupied energy level of an element’s atoms.

The valence electrons determine the chemical properties of an element. Why do you think this would be true?

Atoms in group 3 have 3 valence electrons, atoms in group 17 have 7 valence electrons, etc.

Valenceelectron

To find the number of valence electrons in an atom of a representative element (elements found in the s and p blocks), simply look at its group number.

Valence Electrons

1 2 3 4 5 6 7 8

1 4

There is one exception: helium has only 2 valence electrons.

Number of valence electrons in neutral atoms:


Valence Electrons

Lithium 1s22s1 has 1 valence electron in its outermost,

n=2, energy level.

Oxygen 1s22s22p4 has 6 valence electrons

5 How many valence electrons does potassium have?

A 3

B 1

C

D 4

19

Answer

E 8


6 How many valence electrons does Aluminum have?

A 5

B 7

C 3D 27

E 13

Answer

7 How many valence electrons does Barium have?

A 1

B 2

C 52

D 3

Answer

E 6


8 Arsenic (As) has 6 valence electrons.

True

False

Answer

Ions



Cations are positive and are formed by elements on the left side of the periodic chart (metals).

Ions

Anions are negative and are formed by elements on the right side of the periodic

chart (nonmetals).

Ions are atoms or groups of atoms that have become charged by either gaining or losing electrons.

The Formation of CationsMetals usually give up/lose valence electrons to become

more stable.

This results in a noble gas electron configuration (usually 8 electrons, but 2 in the case of He) in their now outermost shell.

How many electrons does the Na+ ion have?

Na : 1s2 2s2 2p6 3s1 Na +1 : 1s2 2s2 2p6

Loss of valence electrons

Ne atom

1s

2s

2p

3s


The Formation of Cations

Na atom Na+ ion

loses e

11p11e

11p10e

The Na+ ion is smaller than the Na atom. Do you remember what factors cause this reduction in size?

Cations of Group 1A elements always lose 1 electron and have a charge of 1+.

Cations of Group 2A elements always lose 2 electrons and have a charge of 2+.

The Formation of Cations

Mg Mg2+ 2e+

Mg atom(electricallyneutral,

charge = 0)

Mg ion(+2 indicates 2 units of positive

charge)

(2 in front of e indicates 2 units

of negative charge)


Nonmetals usually gain valence electrons. This results in a noble gas configuration of 8 electrons in their outer shell

The Formation of Anions

How many electrons does the Cl have?

Cl 1s22s22p63s23p5 Cl 1s22s22p63s23p6 Ar atom

2s

2p

3s

3p


Cl atom Cl ion

Gains an e17P17e

17p18e

Single anions are named with a shortened element name and an "ide" ending. Cl is named chloride.



Anions of Group 15 elements always gain 3 electrons and have a charge of 3

Anions of Group 16 elements always gain 2 electrons and have a charge of 2

Anions of Group 17 elements always gain 1 electron and have a charge of 1

Consider Group 14 elements, what common charge(s) would you predict for these elements?

Formation of Ions and Metallic Character

The more metallic an element, the easier it loses electrons, resulting in the formation of cations.

The less metallic an element, the greater the hold on electrons, and the less likely they are to form cations.


Ion Symbols

To write the symbol for an ion, write the symbol of the element and show the ion charge as a superscript, with the number value first followed by the + or sign.

Ex: Ca2+

When an ion has a charge of 1+ or 1, it is not necessary to put the 1 in the ion symbol, just the + or sign.

Ex: F1 may simply be written F.

9 Metals tend to __________ electrons and nonmetals tend to __________ electrons. A gain, gainB lose, loseC gain, loseD lose, gainE neither, they keep their electrons

Answer


10 Anions tend to be __________ and cations tend to be __________.

A metals, metalsB nonmetals, nonmetals

C metals, nonmetals

D nonmetals, metalsE metalloids, metalloids

Answer

11 Metals lose electrons to form cations

True

False

Answer

True


12 Anions are formed from nonmetals

True

False

Answer

13 Nonmetals tend to lose electrons forming ions

True

False Answer


14 This is the ion formed from a calcium atom

A Ca+

B Ca2+

C Ca

D Ca2

Answer

15 Phosphorous forms an ion with a charge of __________. A 1+B 2

C 3+

D 3

E 2+

Answer

D


16 Aluminum forms an ion with a charge of __________.

A 2+

B 1

C 3+

D 2

E 0 Answer

17 Of the following, __________ contains the greatest number of electrons.

A P3+

B PC P2

D P3

E P2+

Answer


18 Oxygen forms an ion with a charge of __________. A 2

B 2+

C 3

D 3+

E 6+

Answer

19 Iodine forms an ion with a charge of __________. A 7

B 1+

C 2

D 2+

E 1

Answer


20 This is the ion formed from nitrogen

A N

B N2

C N3+

D N3

Answer

21 Predict the charge of the most stable ion of S? A 3+B 1C 6+D 2+E 2

Answer


22 What would be the expected charge on the gallium (Ga) ion?A +1B +2C +3D +13E 5

Answer


Ionic Bonding



Introduction to Chemical Bonds

Ionic The electrostatic ( positive to negative) attraction between ions

Covalent The sharing of electrons between atoms

Metallic Each metal atom bonds to other metals atoms within a "sea" of electrons (covered in a later unit)

There are three basic types of bonds:


ElectronegativityElectronegativity is how strongly an atom attracts electrons from a neighboring atom.

Electronegativity

Electronegativity increases left to right across the periodic table, and decreases as you move down a column. Flourine is the most electronegative element.

Francium is the least electronegative element.


Atoms with a high electronegativity will be able to attract electrons away from atoms with a much lower electronegativity.

This removal of electrons can occur when the difference in electronegativity between the two atoms is approximately 1.7 or higher.

Once a positive and negative ion are formed, they will be attracted to each other via the electrostatic force.

Ionic Bonding

Ionic Bonding

Neutral atom

7 valence electrons

High Electronegativity

+ Cation Anion

Neutral atom

1 valence electron

Low Electronegativity


Ionic Bonding

The atom with high electronegativy attracts valence electrons from the atom with lower electronegativity.

Generally when a metal reacts with a nonmetal, the metal loses electrons to form a cation and the nonmetal gains electrons to form an anion.

When the atoms become oppositely charged ions the electrostatic force of attraction brings them together.

Electrostatic force of attraction = bond

+ Cation Anion

Compounds composed of cations and anions are called ionic compounds.

Although they are composed of ions, ionic compounds are electrically neutral since the electrons being lost by the metal are the same electrons being gained by the nonmetal.

The electrostatic forces that hold ions together in ionic compounds are called ionic bonds.

Ionic Bonding


Na Cl

Ionic BondsThe electron transfer process in creating an ionic bond:

The dots represents the valence electrons in an atom.

click here for an animation of this reaction

An electronegativity difference of approximately 1.7 can only occur between a metal and a nonmetal.

Ionic Bonding

http://www.visionlearning.com/en/library/Chemistry/1/Chemical-Bonding/55

http://www.visionlearning.com/en/library/Chemistry/1/Chemical-Bonding/55


23 Which pair of atoms will form an ionic bond?

A Li and NeB K and BrC K and CsD S and Cl

Answer

24 Which pair of atoms will form an ionic bond?

A Li and BeB Na and MgC K and CaD Na and Cl

Answer


25 An ionic bond would form between Sc and F?

True

False

Answer

True

26 Which of the following compounds would you expect to be ionic?

A H2OB CO2

C SrCl2D SO2

E H2S

Answer


Properties of Ionic Compounds



1. They are crystalline solids at room temperature The cations and anions are arranged in a repeating

geometric pattern.


2. They have high melting points due to the strength of the ionic bonds.

3. They conduct electricity when melted (molten) or dissolved in water (aqueous) due to the ability of the ions to move around.


A chemical formula shows the kinds and numbers of atoms in the smallest representative unit of a substance.

A formula unit is the lowest wholenumber ratio of ions in an ionic compound. This is also called the empirical formula.

Formula Units


Chemical formulas

Chemical formulas are written using the chemical symbol followed by a subscript indicating the number of that atom or ion.

NaCl indicates a ratio of 1 Na+ : 1 Cl

H2O indicates a ratio of 2 H : 1 O

Predicting an Ionic Compound's Formula



Predicting an Ionic Compound FormulaPotassium (K) with an electronegativity of 0.8 and oxygen (O) with an electronegativity of 3.5 will form an ionic compound.

What is the formula for an ionic compound of potassium and oxygen?

KO

K

How many additional valence electrons does oxygen need? 2

How many valence electrons does potassium have? 1

How many potassium atoms will it take to give oxygen the electrons it needs? 2

The formula unit is K2O

The metal is always first in the formula, followed by the nonmetal.

Predicting an Ionic Compound Formula

What is the formula for an ionic compound of Mg and N?

How many additional valence electrons does N need? 3

How many valence electrons does Mg have to offer? 2

How many Mg atoms will it take to give how many N the electrons it needs? (Find the lowest common multiplier first.)

MgN

NMg

Mg

3 Mg : 2 N

The formula unit is Mg3N2


MgN

NMg

Mg

Ionic compounds are neutral

As you can see in the diagram, all electrons lost by a Mg must be taken by a N.

This causes the total positive charge (electrons lost) to be equal to the total negative charge (electrons gained).

Example: Write the formula for calcium sulfide.

Step 1: Identify the cation & write its common ion

Calcium is in group 2: Ca2+

Step 2: Identify the anion & write its formula

Sulfur is in group 6: S2

Step 3: Only one cation and one anion are needed to make a neutral compound.

Step 4: The formula is written CaS

Predicting an Ionic Compound Formula


27 The formula for barium sulfide is Ba2S2 .

True

False

Answer

28 The formula for the ionic compound between Mg and S is:

A Mg2S2

B MgS

C MgS2

D SMg

E I don't know how to do this.

Answer


29 The formula for the ionic compound between Cs and O is:

A CsO2

B OCs2C Cs2O

D OCs2

E I don't know how to do this. Answer

30 The ionic compound formed between Ca and N is:

A CaN

B Ca2N2

C Ca3N2

D Ca2N3

E I don't know how to do this.

Answer


31 The ionic compound formed between Al and O

A Al3O2

B Al2O3

C AlO

D Al2O2


32 What is the ionic compound formed between Ca and Al?

A CaAl

B Ca3Al2C Al2Ca3

D No compound is formed.

Answer


33 What is the ionic compound formed between P and Br?

A P3Br

B BrP

C This compound is not considered ionic

D (BrP)2E I don't know how to do this.

Answer

34 What is the formula for sodium phosphide?

A SP3

B NaP

C Na3P

D NaP3



35 What is the formula for strontium bromide?

A SrBr

B SrBr2

C Sr2Br

D BrSr2

Answer


Naming Ionic Compounds


Naming Binary Ionic Compounds Cations

Charge Formula Name

+1

+2

+3

H+ Li+ K+ Cs+ Ag+

Mg2+ Ca2+ Ba2+ Cd2+

Al3+

Hydrogen ionLithium ionPotassium ionCesium ionSilver ion

Magnesium ion Calcium ion Barium ion Cadmium ion

Aluminum ion

Many cations have the same name as the original, neutral atom.


All monoatomic anions end in "ide".

Nitride N3

Phosphide P3

Oxide O2

Sulfide S2

Fluoride F

Chloride Cl

Bromide Br

Iodide I

Group 15 Group 16 Group 17

Naming Binary Ionic Compounds Anions

Binary (twoelement) compounds are named by writing the name of the cation followed by the name of the anion.

The name of the cation is the same as the metal name.

The name of the anion is the name of the nonmetal with the suffix changed to ide.

Naming Binary Ionic Compounds

Examples:

NaCl = sodium chlorideKI = potassium iodideLi2S = lithium sulfide


36 The correct name for Na2S is

A Sodium sulfateB Sodium sulfideC Disodium sulfideD Sulfur nitride

Answer

37 The correct name for SrO is __________.

A strontium oxide B strontium hydroxide C strontium peroxide D strontium monoxide E strontium dioxide

Answer


38 The correct name for Al2O3 is __________.

A aluminum trioxide B dialuminum oxide C dialuminum trioxide D aluminum oxide E aluminum hydroxide

Answer


Names and Formulas of Ionic Compounds with Transition Metals



Recall that sblock metals and some p block elements like aluminum have only one possible ionic charge, based on the Octet Rule.

However, most transition metals (d block elements) can form more than one type of cation with different charge.

Sn, Pb from the pblock are called posttransition metals and will form more than one type of ion and behave like transition metals.

Cations formed by Transition Elements

Cations formed by Transition Elements

The 2+ charge is very common among the transition metals since they lose their two "s" electrons first, before losing others from their "d" orbital.

http://philschatz.com/chemistrybook/contents/m51186.html

http://philschatz.com/chemistry-book/contents/m51186.html


Cations Formed by Transition ElementsOnly common transition metals are shown.

Silver, cadmium and zinc only form one cation, Ag+ , Cd2+ and Zn2+

Note the two mercury cations, one is a single atom, the other is made up of two atoms together this is called a polyatomic ion.

Silver, Zinc, and Cadmium IonsWhy do these ions only have one possible charge?

Let's look at their electron configurations.

The "d" orbital of both zinc and cadmium are full and therefore very stable so the only electrons it will lose are the two "s" electrons...

Zn: [Ar]4s23d10 Zn2+: [Ar]3d10

The "d" orbital is also full with silver as it has largely taken an electron from it's own "s" orbital to make stabilize the "d" orbital. Therefore, it only has 1 electron left to lose.

Ag: [Kr]5s14d10 Ag+ : [Kr]4d10


Cations formed by Transition ElementsWe will use the Stock naming system. The name of the transition metal MUST be followed by Roman Numerals indicating its charge.

Formula Name

Cu+1 Copper (I) ion

Co+2 Cobalt (II) ionFe+2 Iron (II) ionMn+2 Manganese (II) ionPb+2 lead (II) ion

Cr+3 Chromium (III) ionFe+3 Iron (III) ion

What would be the names of Cu 2+ and Mn 7+?

Writing Formulas with Transition Metals

The charge on the cation is indicated by the Roman numeral, as shown in this example.

Fe2O3

Reduce if necessary.

Write ion formulas.

Determine ratio of cations to anions.

Fe3+ O2

Iron (III) oxide


Writing Formulas with Transition Metals

The charge on the cation is indicated by the Roman numeral, as shown in this example.

Tin (IV) oxide

Write ion formulas.

Determine ratio of cations to anions.

Reduce if necessary.SnO2

Sn2O4

Sn4+ O2

39 Which metal is capable of forming more than one cation?

A KB CsC BaD AlE Sn

Answer


40 Which metal is not capable of forming more than one cation?

A Cu

B Au

C Fe

D Sn

E Al

Answer

Naming a Compound with a Transition Metal

In order to correctly name a formula containing a transition metal, it is necessary to first determine the charge on the cation.

Since all compounds are neutral, the total positive cation charge must equal the total negative anion charge AND since anion charges don't vary, we can use this formula to find the charge on the transition metal.

Total cation charge + Total anion charge = 0

(charge of cation) (# of cations) + (charge of anion) (# of anions) = 0


Example Formula with Transition Metals

In the case of FeCl3 , we know there is 1 Fe and 3 Cl, and the charge on Chloride is always 1.

Fill in these values and solve for the charge on Fe.

(charge of cation) (# of cations) +(charge of anion) (# of anions) = 0

(x) (1) + (1) (3) = 0

So x = 3 and the cation is Fe3+ .The compound is Iron (III) Cloride

Formulas with Transition Metals

Cr1 O1

Cr2+ O2

CrO: Determine the charge of O.

Since O has charge of 2, Cr must have a charge of 2+

Cr2O2

Chromium (II) Oxide

Here's another practice problem.


41 The correct name of the compound V2O3

is vanadium(II)oxide.

True

False

Answer

42 The correct name for Cu3N is:

A copper nitrideB copper (I) nitrideC copper (II) nitrideD copper(III)nitrideE copper(III) nitrogen

Answer


43 The name of FeCl3 is

A iron chlorideB iron (II) chlorideC iron (III) chlorideD iron(I)chloride

Answer

44 The correct formula for tin (IV) oxide is:

A SnO2B SnOC Sn4O4D Sn4O2

Answer

A


45 The formula for copper (II) sulfide is

A CuS2

B CuS C Cu2 S2

D (CuS)2

Answer

E Cu2S

46 Which one of the following compounds is copper(I) chloride?

A CuCl

B CuCl2C Cu2ClD Cu2Cl2E Cu3Cl2 A

nswer


47 The charge on the cation in the salt Fe2O3 is __________.

A 1+B 2+

C 3+

D 5

E 6 Answer

48 What is the charge on zirconium ion in ZrO2 ?

A 2+

B 4+

C 1+D 2

[*]

E 3+

Answer


Polyatomic Ions


A polyatomic ion is a group of atoms bonded together that have a charge and acts like a single unit or ion. They are commonly part of an ionic compound, as either the cation or the anion.

Sulfate = (SO4)2

Nitrate = (NO3)

Carbonate = (CO3)2

When writing formulas for compounds containing polyatomic ions, use ( ) to keep the atoms together.

Do not change the subscripts inside the "( )"

Polyatomic Ions


Most of the polyatomic ions contain oxygen atoms.

Many anions names end with “ite” or “ate”

In “ite/ate” pairs, the ion with fewer oxygen atoms will have the “ite” ending

Examples: sulfite /sulfate nitrite /nitrate

Note that the suffix does not indicate the actual number of O atoms.

Polyatomic Ions


Polyatomic Ions

Familiarize yourself with the polyatomic ions on your reference sheetBe careful of ide, ite, and ate!

H+ = proton or hydrogen ion

or bicarbonate

]

.

Formulas and Names of Ionic Compounds with

Polyatomic Ions (Ternary Ionic Compounds)



Writing Formulas for Ternary Ionic Compounds

Ternary ionic compounds, compounds that contain 3 or more elements, are neutral, just like binary ionic compounds. Therefore, the goal is to find the lowest ratio of cations to anions that will yield a neutral compound.

This ratio is represented in a formula unit.

Examples of formula units

CaCO3 Zn(C2H3O2 )2

AgNO3 Na2SO3


To write a formula

Example: Write the formula for lithium phosphate.

Step 1: Identify the cation & write its formula

Lithium is in group 1 > Li+

Step 2: Identify the anion & write its formula

Phosphate is a polyatomic ion > PO43

Step 3: Find the ratio of cation to polyatomic anion

Li3(PO4)1 or simply Li3(PO4)



Example 1: Write the formula for

lithium chlorate.

Li+1 (ClO3)1

= Li(ClO3)

= LiClO3

Note: The ( ) are removed because only 1 chlorate ion is present.

Example 2: Write the formula for manganese(III) carbonate.

Mn3+ (CO3)2

= Mn2(CO3)3

Note: The ( ) are needed here because more than one carbonate ion are present

Move for AnswerMove for Answer

49 The formula for aluminum phosphate is:

A AlPO4

B Al3 (PO4 )

C Al2 (PO4 )3

D Al3 (PO4 )3

Answer


50 What would be the correct formula for cobalt(III) carbonate?

A Co3CO3B Co2CO3

C Co2(CO3)3D Co3(CO3)2E CoCO3

Answer

51 The formula for sodium hydroxide is

A Na (OH)2 B NaOH

C Na(OH2 ) D Na(HO)

E NaOH2

Answer


52 The formula for calcium sulfate is

A CaSO4 B Ca2 (SO4 )2C Ca(SO3 ) D Ca2 (SO3 )2

E CaS

Answer

53 How many nitrate ions are present in the formula of aluminum nitrate? (Write the formula first to find out.)

A 1B 2C 3D 4E 5

Answer


54 How many total ions (cations and anions) are present in the formula of lithium acetate?

A 1B 2C 3D 4E 5

Answer

Writing Formulas for Ionic CompoundsComplete the table by filling in the formula for the ionic compound formed by each pair of cations and anions, as shown for the first pair.


Write the formula for the following compounds:

1. Magnesium iodide MgI2

2. Calcium sulfite CaSO3

3. Barium hydrogen carbonate Ba(HCO3)2

4. Iron (III) phosphate FePO4


Move for answer

Ternary ionic compounds contain three or more different elements due to the presence of polyatomic ion(s).

Just as in binary ionic compounds, the name of the cation is given first, followed by the name of the anion.

Names of ternary compounds often end in ite or ate.Examples

CaCO3 calcium carbonate Zn(C2H3O2 )2 zinc acetateAgNO3 silver nitrateNa2SO3 sodium sulfite

Naming Ternary Ionic Compounds

Move for answer


55 The correct name for NaClO is

A sodium chlorate

B sodium chloride

C sodium chlorite

D sodium chloride oxide

E sodium hypochlorite

Answer

56 Mg(HCO3 )2 is

A Magnesium carbonate

B Magnesium hydrogen carbonate

C Magnesium hydroxide

D Magnesium carboxide E Magnesium dibicarbonate A

nswer


57 Ammonium carbonate is

A NH4CO3

B (NH4 )2CO3

C NH4 (CO3 )2

D (NH4 )2CO2

Answer

Naming Ternary Ionic CompoundsIf the formula involves a transition or post transition element, you must first deduce the charge so it can be included in the name.

For example: Name Cu2CO3

1. Determine the charge of the polyatmoic anion CO3, which is 2

Cu2 (CO3)2

2. Determine the charge of the cation, Cu carries a +1 charge

This compound is called copper(I) carbonate


58 What is the name for Ga2(SO3)3?

A gallium sulfite

B gallium (I) sulfiteC gallium (III) sulfiteD gallium (III) sulfate

Answer

59 Which is the name for AuF3?

A gold (I) flourideB gold(III) flourideC gold flourideD gold flourineE gold triflouride

Answer


60 What is the name for Sn(CO3)2?

A tin carbonateB tin(II) carbonateC tin carbideD tin tetracarbonateE tin (IV) carbonate

Answer

E

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