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4 years ago

Explain how the periodic table can help in writing electron configurations

2 answers:

4 0

The periodic table can help in writing electron configurations because on the periodic table, you might notice a number in the top right corner, this tells you how much electrons are in the specific element....please mark brainliest!

Vinil7 [7]4 years ago

3 0

Look At the bottom number

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104. Fill in the blanks to complete the table.

iren2701 [21]

Explanation:

Just a few things to remember:

# of neutrons = Mass number - # protons
Mass number = # protons + # neutrons
Atomic Number = # of protons
# of electrons = # of protons - charge on the atom
Symbol - use the atomic number to find the element in the periodic table

3 0

3 years ago

The formula weight of a compound is determined by adding up the individual weights of every _______ in that compound.

Jlenok [28]

Answer:

C. Atom

The formula weight is calculated by the sum( adding) of the atomic masses for every atom in the formula

3 0

3 years ago

A __________ is a natural or human-made body of water surrounded by land.

Sophie [7]

Answer:

Lake

Explanation:

Yeah...not much else to say honestly

5 0

3 years ago

Identify the oxidized substance, the reduced substance, the oxidizing agent, and the reducing agent in the redox reaction. Cu(s)

spin [16.1K]

Answer: Copper is getting oxidized and is a reducing agent. Silver is getting reduced and is oxidizing agent.

Explanation:

Oxidation reaction is defined as the reaction in which an atom looses its electrons. Here, oxidation state of the atom increases.

$X\rightarrow X^{n+}+ne^-$

Reduction reaction is defined as the reaction in which an atom gains electrons. Here, the oxidation state of the atom decreases.

$X^{n+}+ne^-\rightarrow X$

Oxidizing agents are defined as the agents which oxidize other substance and itself gets reduced. These agents undergoes reduction reactions.

Reducing agents are defined as the agents which reduces the other substance and itself gets oxidized. These agents undergoes reduction reactions.

For the given chemical reaction:

$Cu(s)+2AgNO_3(aq.)\rightarrow 2Ag(s)+Cu(NO_3)_2(aq.)$

The half reactions for the above reaction are:

Oxidation half reaction: $Cu(s)\rightarrow Cu^{2+}(aq.)+2e^-$

Reduction half reaction: $2Ag^+(aq.)+2e^-\rightarrow 2Ag(s)$

From the above reactions, copper is loosing its electrons. Thus, it is getting oxidized and is considered as a reducing agent.

Silver is gaining electrons and thus is getting reduced and is considered as an oxidizing agent.

4 0

4 years ago

What is the oxidized substance in the following reaction? Fe + 2HCl → FeCl2 + H2

LenKa [72]

Fe⁰ + 2 H⁺¹Cl⁻¹ = Fe⁺²Cl₂⁻¹ + H₂⁰

the iron is oxidized

the hydrogen is reduced

hope this helps!

4 0

3 years ago