a. alkali metals b. alkaline earth metals c. halogens d. noble gases e. none of the above 3. What is the collective term for the elements in Groups 1, 2, 13-18? a. actinide series b. lanthanide series c. rare earth elements d. representative elements e. transition elements 4. What is the collective term for the elements in Groups 3-12? a. actinide series b. lanthanide series
4) When naming an ionic compound, which ion is given first? The metal ion is named first 5) Give explanations for the following: a. Argon will not react with any other element It already has a complete number of eight, a full number in its valance shell so it cannot react with itself or another element b. The reaction between sodium chloride gives out a lot of heat and light. The chemical energy of the product is less then the chemical energy of the reactants. This energy is indestructible and is converted to light and heat.
Name: ___________________________________ Date: ______________ Practice Test #3 ____ 1. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these 2. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 3.
However, in many instances, no precipitate forms because the recombination of ions yields only soluble compounds. In this experiment you will mix together solutions containing various dissolved ions to determine how the solubility rules listed in Table F were created. Pre-lab questions: 1. Explain, on the particle level, what happens to ionic compounds when they dissolve in water? [1 pt] Ionic compounds dissociate when it dissolve in water.
There will have some error. 2) A volatile liquid was allowed to evaporate in a 43.298 g flask that has a total volume of 252 ml. the temperature of the water bath was 100˚C at the atmospheric pressure of 776 torr. The mass of the flask and condensed vapor was 44.173 g. calculate the molar mass of the liquid. T = 273 + 100 = 373 V = 252 mL = 1 L / 1000 mL = 0.252 L P = 776 Torr R= 0.0821 mass of 44.173 - 43.298 g = 0.875g moles of gas = PV / RT = 776 x .252 / 62.363 x (273+100) =0.00841 moles molar mass = 0.875g / 0.00841 moles = 104.1 g/
When the hydrate is heated, it easily loses water molecules attached and becomes an anhydrous salt. The corresponding chemical reaction for hydrated magnesium sulfate can be written as |MgSO4•7H2O ( MgSO4 + 7H2O |(1) | where MgSO4 is the anhydrous salt. Usually,
A) sulfide ion B) sulfate ion C) sulfite ion D) bisulfate ion 12. What is the correct chemical formula of tin(IV) cyanide? A) Ti(CN) 4 B) TiC 4 N 4 C) Sn(CN) 4 D) SnC 4 N 4 E) Sn(CN) 2 Page 3 13. The formula for zinc acetate is _____. A) ZnCH 3 CO 2 B) Zn(CH 3 CO 2 ) 2 C) Zn(HCO 3 ) 2 D) Zn(HCl) 8 14.
1. Equations for each reaction in the preparation. (a) Reaction of copper (II) oxide with nitric acid. CuO (s) + 2HNO3 (aq) → Cu(NO3)2 (aq) + H2O (l) (b) Neutralization of the excess nitric acid with sodium carbonate. Na2CO3 (s) + 2HNO3 (aq) → 2NaNO3 (aq) + CO2 (g) + H2O (l) (c) Reaction of aqueous copper(II) nitrate with sodium carbonate.