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posledela
3 years ago
7

Why isn't hydrogen considered an alkali metal ?

Chemistry
2 answers:
vovikov84 [41]3 years ago
7 0
Hydrogen is a non-metal, it is one of the two elements on the periodic table that only need two valence electrons to be stable. Hydrogen doesn't share many properties with the other Alkali Metals. It has a much higher electronegativity, doesn't form ionic bonds, doesn't react with the same things that the other elements in group one do (like water.) The only reason hydrogen is place there is because it has one valence electrons like all the other alkali metals and there is not where else to place hydrogen, because it doesn't really fit in with any group. 
Maurinko [17]3 years ago
4 0
<span>Hydrogen isn't classified as an alkali metal because it exhibits several properties that are not found in the alkali metal group, including the tendency to be found as a diatomic molecule, a tendency to form weak bonds with other bound hydrogen atoms nearby, weak electromagnetism, a low activity series placement, and the tendency to be found as a gas. Because of all this, it's impossible to classify it with any group, although it does seem to be closest to nonmetals.</span>
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Abuse of time and temperature can occur in each of the following ways except: The items are not cooked to the proper internal te
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Holding items in the freezer for too long is not an example of abuse of time and temperature.

<h3>What is abuse of time and temperature?</h3>

Abuse of time and temperature has to do with a situation in which time is used in an improper way or food is not held at the correct temperature ultimately leading to food poisoning.

Holding items in the freezer for too long is not an example of abuse of time and temperature.

Learn more about temperature: brainly.com/question/7510619

5 0
2 years ago
Explain why lithium is a strong reducing agent, whereas fluorine is a strong oxidizing agent.
Tom [10]
Lithium is a good reducing agent because it is electropositive [it rapidly gains electrons]
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3 0
3 years ago
Suppose of copper(II) acetate is dissolved in of a aqueous solution of sodium chromate. Calculate the final molarity of acetate
uranmaximum [27]

Answer:

0.0714 M for the given variables

Explanation:

The question is missing some data, but one of the original questions regarding this problem provides the following data:

Mass of copper(II) acetate: m_{(AcO)_2Cu} = 0.972 g

Volume of the sodium chromate solution: V_{Na_2CrO_4} = 150.0 mL

Molarity of the sodium chromate solution: c_{Na_2CrO_4} = 0.0400 M

Now, when copper(II) acetate reacts with sodium chromate, an insoluble copper(II) chromate is formed:

(CH_3COO)_2Cu (aq) + Na_2CrO_4 (aq)\rightarrow 2 CH_3COONa (aq) + CuCrO_4 (s)

Find moles of each reactant. or copper(II) acetate, divide its mass by the molar mass:

n_{(AcO)_2Cu} = \frac{0.972 g}{181.63 g/mol} = 0.0053515 mol

Moles of the sodium chromate solution would be found by multiplying its volume by molarity:

n_{Na_2CrO_4} = 0.0400 M\cdot 0.1500 L = 0.00600 mol

Find the limiting reactant. Notice that stoichiometry of this reaction is 1 : 1, so we can compare moles directly. Moles of copper(II) acetate are lower than moles of sodium chromate, so copper(II) acetate is our limiting reactant.

Write the net ionic equation for this reaction:

Cu^{2+} (aq) + CrO_4^{2-} (aq)\rightarrow CuCrO_4 (s)

Notice that acetate is the ion spectator. This means it doesn't react, its moles throughout reaction stay the same. We started with:

n_{(AcO)_2Cu} = 0.0053515 mol

According to stoichiometry, 1 unit of copper(II) acetate has 2 units of acetate, so moles of acetate are equal to:

n_{AcO^-} = 2\cdot 0.0053515 mol = 0.010703 mol

The total volume of this solution doesn't change, so dividing moles of acetate by this volume will yield the molarity of acetate:

c_{AcO^-} = \frac{0.010703 mol}{0.1500 L} = 0.0714 M

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3 years ago
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The specific heat for liquid ethanol is 2.46 J/(g•°C). When 210 g of ethanol is cooled from
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Answer:

a) heat it from 23.0 to 78.3

q = (50.0 g) (55.3 °C) (2.46 J/g·°C) =  

b) boil it at 78.3

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c) sum up the answers from the two calculations above. Be sure to change the J from the first calc into kJ

Explanation:

3 0
3 years ago
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