particular metal ion. A very common hydrate often encountered in the general chemistry laboratory is copper (II) sulfate pentahydrate‚ CuSO4.5H20. The word “pentahydrate” in the name of this substance indicates that five water molecules are bound in this substance per copper sulfate formula unit. Hydrated water molecules are generally indicated in formulas as shown above for the case of the copper sulfate‚ using a dot to separate the water molecules from the formula of the salt itself. Although not usually
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Scientific at scientificsonline.com Add one scoop each of luminol and perborate mixtures and a few copper sulfate crystals to each cup. Add a consistent amount of each chemical. Try to count the grains of copper sulfate so that you are adding close to the same amount to each reaction. As an option‚ premix the dry ingredients in a clean‚ dry container. Add enough luminol‚ perborate‚ and copper sulfate for 10 reactions. This will minimize variation that could result if you add them separately. Put the
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Oxidation-Reduction Activity Series 1 Copper (II) Sulfate‚ 1 M - 3 mL in Pipet 1 Iron (III) Chloride‚ 2 M - 3 mL in Pipet 1 Iron Metal‚ 2 pc in Bag 2"x 3" Magnesium Metal (ribbon) - 2 Small Pieces in Bag 2"x 3" 1 Magnesium Sulfate‚ 2 M - 3 mL in Pipet 1 Lead metal‚ 4 small pieces in bag 2 x 3” 1 Sodium Sulfate‚ 1 M - 3 mL in Pipet 1 Zinc Metal - 2 Small Pieces in Bag 2"x 3" 1 Zinc Nitrate‚ 2 M - 3 mL in Pipet Procedure 1. Get all the materials 2. Place 10 drops of Sodium sulfate‚ Na2SO4 into well A1
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HKDSE CHEMISTRY – A Modern View (Chemistry) Coursebook 3 Suggested answers |Chapter 25 Simple molecular substances with non-octet |Page Number | |structures and shapes of simple molecules | | |Class Practice |1 | |Chapter Exercise
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Metals using different Solutions Purpose/ Hypothesis: The purpose of this lab was to clearly identify the reactivity of magnesium‚ zinc and copper. The metals reactivity will be exemplified as it will be tested with different solutions such as zinc sulfate (ZnSO4)‚ copper sulfate (CuSO4)‚ hydrochloric acid (HCL)‚ magnesium sulfate (Mg2SO4)‚ iron (II) sulfate (FeSO4) and tin (II) chloride (SnCl2). This will allow us in creating an activity series to visually see the reactivity when given single displacement
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tube rack Part 2: The materials are found on page 161 in the textbook Sciencepower 9 Part 3: The materials are found on page 161 in the textbook Sciencepower 9 Part 4: 100 mL Beaker; Hot plate; Beaker tongs; Wire gauze; Copper [II] sulfate ………………solution [aq]; 1 Plastic pipette Part 5: The materials are found on page 162 in the textbook Sciencepower 9 Part 6: The materials are found on page 162 in the textbook Sciencepower 9 Part 7: Test tube; Test tube rack;
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hydrated copper (II) sulphate compound? Controlled Variable: The mass of hydrated copper (II) sulphate. Responding Variable: The mass of dehydrated copper (II) sulphate‚ mass of H2O Materials: Ones on the handout + Hot plate. Procedure: 1. Mass 3.00g of hydrated copper (II) sulphate using electronic balance 2. Measure the mass of a thin‚ crucible dish using electronic balance 3. Gently pour hydrated copper (II) sulphate into the crucible dish 4. Heat the hydrated copper (II)
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Binary Compounds w/ Fixed Charge Given The Formula‚ Write The Name Binary Compounds w/ Fixed Charge Given The Name‚ Write The Formula Binary Compounds w/ Variable Charge: Stock System Given The Name‚ Write The Formula Binary Compounds w/ Variable Charge: Stock System Given The Formula‚ Write TheName 1) MgO 2) LiBr 3) Ca3N2 4) Al2S3 5) KI 6) SrCl2 7) Na2S 8) RaBr2 9) MgS 10) AlN 11) Cs2S 12) KCl 13) Sr3P2 14) BaI2 15) NaF 16) CaBr2 17) BeO 18) SrS 19) BF3 20) AlP 21) Rb2O 22) CaI2
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parentheses‚ followed by the name of the element‚ is used for elements that can form more than one positive ion. This is usually seen with metals. You can use a chart to see the possible valences for the elements. Fe2+ Iron (II)Fe3+ Iron (III)Cu+ Copper (I)Cu2+ Copper (II) -ous and -icAlthough Roman numerals are used to denote the ionic charge of cations‚ it is still common to see and use the endings -ous or -ic. These endings are added to the Latin name of the element (e.g.‚stannous/stannic for tin) to
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Chapter Exercise 33 Chapter 34 Importance of redox reactions in modern ways of living Class Practice 36 Chapter Exercise 37 Part Exercise 39 Chapter 35 Energy changes in chemical reactions Class Practice 42 Chapter Exercise 43 Chapter 36 Standard enthalpy change of combustion‚ neutralization‚ solution and formation Class Practice 44 Chapter Exercise 46 Chapter 37 Hess’s Law Class Practice 48 Chapter Exercise 51 Part Exercise 53 Chapter 25 Simple molecular substances with non-octet structures and
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