Chemistry chapter 9 section 2

Nickle(ii) hydroxide(s) decomposes to produce nickle(ii) oxide(s) and water.

2Ni (OH)2(s) -> 2NiO + 2H2O

K(s) + ZnCl2(aq) ->

2k +ZnCl2 -> 2KCl + 2N, a Single-replacement reaction has occurred.

Cations

A and B represent positively changed ions

Synthesis reaction

A chemical reaction in which two or more substances react to produce a single product.

Write out the generic formula the represents a decomposition reaction.

AB -> A+B

Aqueous sodium oxalate and aqueous lead(ii) nitrate react to produce solid lead(ii) oxalate and aqueous sodium nitrate.

Na2C2O4(aq) + Pb (No3) -> Pb C2 O4 + 2Na (No3)

The gases nitrogen dioxide and oxygen react to produce dinitrogen

No2(g) + O2(g) -> N2O5(g) = 4No2(g) + O2(g) -> N2O5(g), both

Replacement reaction

The replacement of an element in a compound.

Steps for writing Double-replacement reactions

1. Write the components of the reactions in the skeleton equation. 2. Identify the action and the anions I'm ecah compound. 3. Pair up each cation with the anion from the other compound. 4. Write the formulas for the products using the pairs from step 3. 5. Write the complete equation for the double-replacement reaction. 6. Balance the equation.

Write the generic formula that represents a synthesis reaction.

A+ B -> AB

Generic formula for single-replacement reaction

A+Bx -> Ax + B

The solids aluminum and sulfur react to produce aluminum sulfide.

Al(s) + S(s) -> Al2S3(s), Synthesis

Generic equation for a double replacement reaction

Ax +By -> Ay + Bx

Aqueous barium chloride and aqueous potassium carbonate react to produce solid barium carbonate and aqueous potassium chloride.

BaCl2(aq) + K2(co3) -> Ba (co3)(s) + 2 KCl(aq)

Write out two examples of combustion reactions

C(s) + O2(g) -> CO2(g) CH4(g) + 2O 2(g) + 2H2O(g)

Fe(s) + Na3PO4(aq)

Fe + Na3Po4, no reaction

4 types of chemical reactions

Synthesis, Combustion, Ecompostition, Replacement

Look at table 4

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Water and dinitrogen pentoxide gas react to produce aqueous hydrogen nitrate.

4No2(g) + O2(g) -> 2N2O5(g), Synthesis

Aluminum oxide(s) decomposes when electricity passes through it.

AlO3 -> Al + O3

Write out two examples of synthesis reactions

CaO(s) + H2O(I) -> Ca(OH)2(s) 2SO2(g) + O2(g) -> 2So3(g)

Cl2(g) + HF(aq) ->

Cl2 + HF, no reaction

Which group on the periodic table is frequently involved in nonmetal replaces nonmetal replacement reactions?

Halogens

Double-replacement reaction

Involves an exchange of ions between two compounds

Write out the two examples of decomposition reactions given on page 292

NH4 NO3(s) -> 2Na(s) + 3N2(g) 2NaN3(s) -> Na(s) + 3N2(g)

Combustion reaction

Oxygen combines with a substance and releases energy in the form of heat and light

Describe the 4 types of chemical reactions and their characteristics.

Synthesis- when two or more substances combine to form one product. Decomposition-when one substance breaks down into two or more substances. Combustion- occurs between hydrogen and oxygen when hydrogen is heated. Replacement reactions- single-replacement reaction, and double-replacement reactions.

Explain how an activity series of metals is organized.

The activity series of metals is the arrangement of matalic elements from the active to the least active.

Can reactions be classified as more than one type? Why or why not?

Yes, a synthesis can also be a combustion reaction.

Two types of replacement or displacement reactions-

1. Single-replacement reaction 2. Double-replacement reaction

Single-replacement reaction

A reaction in which the atoms of one element replace the atoms of another element in a compound.

The two substances (Lil(aq), AgNo3 (aq)) react to produce solid silver iodide and aqueous lithium nitrate.

LiI(aq) + Ag(No3)(aq) -> AgI(s) + Li (No3) (aq)

All double replacement reactions produce with________, a ___________ or a_________.

Water, precipate, gas

Decomposition reaction

When a single compound breaks down into two or more elements or new compounds.

Anions

X and y represent negatively charged ions