3.4 For each of the following elements, locate it in the Periodic Table, and indicate whether it is a metal, metalloid, or non-m
1 answer:
According to its location in the periodic table:
- Ge: Period 4, Group 14. Metalloid.
- Se: Period 4, Group 6, Non-metal.
- Be: Period 2, Group 2, Metal.
It is a table in which elements are ordered in Groups (columns) and Periods (rows).
According to their ubication and properties they can be classified in:
- Metals: occupy the left and center of the table.
- Metalloids: occupy the right of the table (dark green in the attached table).
- Non-metals: occupy the right of the table (yellow and light green in the attached image).
Let's locate and classify the following elements:
- Germanium: Period 4, Group 14. Metalloid.
- Selenium: Period 4, Group 6, Non-metal.
- Beryllium: Period 2, Group 2, Metal.
Learn more about the periodic table here: brainly.com/question/14514242
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Answer:
The standard cell potential is 1.40 V. The correct option is the option D (+1.40 V)
Explanation:
Oxide-reduction reactions, also called redox, involve the transfer or transfer of electrons between two or more chemical species. In these reactions two substances interact: the reducing agent and the oxidizing agent.
An oxidizing element or oxidizing agent is one that reaches a stable energy state as a result of which the oxidant is reduced and gains electrons. The oxidizing agent causes oxidation of the reducing agent generating the loss of electrons of the substance and, therefore, oxidizes in the process.
In other words, the oxidizing agent is that chemical species that in a redox process accepts electrons released by the reducing agent and, therefore, is reduced in said process. The oxidizing agent is reduced because, upon receiving electrons from the reducing agent, a decrease in the value of the charge or oxidation number of one of the atoms of the oxidizing agent is induced .
Electrochemical cells, galvanic cells or batteries are called devices that are capable of transforming chemical energy originated in a spontaneous redox process into electrical energy.
The cellular potential is generally in standard conditions, that is, 1 M with respect to solute concentrations in solution and 1 atm for gases.
In this case you have the reaction:
3 Cl₂(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe³⁺(aq)
In this case the following half-reactions occur:
Semi-reaction of oxidation ( an atom or group of atoms loses electrons, or increases its positive charges): Fe³⁺(aq) + 3 e- -->Fe(s); E⁰ = -0.04 V
Semi-reaction of reduction (an atom or group of atoms gains electrons, increasing its negative charges): Cl₂(g) + 2 e- --> 2 Cl-(aq); E⁰=1.36 V
In an electrochemical cell at 25°C the potentials of the semi-reactions are usually measured in the sense of reduction and generally the standard potential between both electrochemical cells will be:
E⁰=1.36 V - (-0.04 V)
E⁰=1.36 V + 0.04 V
<em>E⁰=1.40 V</em>
<em><u>The standard cell potential is 1.40 V. The correct option is the option D (+1.40 V)</u></em>
Answer:
Explanation:
The atom X has 1 1 protons (atomic number) and thus would have 11 electrons. This means the atom X would have 1 valence electron in it's outermost shell. While the atom Y has 17 protons (atomic number) and thus would have 17 electrons. This means the atom Y would have 7 electrons in it's outermost shell.
The type of bond this atoms (X and Y) would form is an Ionic (or electrovalent) bond. <u>This bond/combination involves the transfer of electron(s) and a molecule is not formed</u> as seen in the image below.
