Use the periodic table to predict the most stable oxidation state for the following element: F...

Use the periodic table to predict the most stable oxidation state for the following element: F

+1

+2

+3

-1

-2

Expert Solution

From the position of F in the periodic table, it can be observed that it possesses the highest electronegativity in the period. Moreover, being the first halogen, it also has the highest electronegativity in the group, making it the most electronegative atom in the periodic table. This, combined with the electronic configuration of 1s² 2s² 2p⁵ of F, makes it possess very low electron-low gain enthalpy as accepting one more electron helps it attain the noble gas configuration of Ne as 1s² 2s² 2p⁶. However, if it were to accept one more electron, owing to high effective nuclear charge in the nucleus, the dianion will be destabilized by high interelectronic repulsions arising from closely residing extra electrons. Taking a deeper look into the electron-affinity and electronegativity of F, it can be said that it is almost impossible to extract even a single electron from the atom, which also correlates with its high first ionization energy. Therefore, it can be concluded that the most stable oxidation state that F can possess is -1.

queen_honey_blossom answered 1 year ago

Match each element in the left column with its most likely oxidation state in a compound...

Match each element in the left column with its most likely oxidation state in a compound in the right column. (Based on the elements location in the periodic table.) __Magnesium A. +1 __Aluminum B. +2 __Oxygen C. +3 __Chlorine D. 0 __Potassium E. -1 __Barium F. -2 __Nitrogen G. -3 __Sulfur H. +4/-4 __Flourine __Strontium __Carbon __Arsenic

Use the group structure of the periodic table and the octet rule to predict the empirical...

Use the group structure of the periodic table and the octet rule to predict the empirical formulas and the molecular geometries for the binary compounds that hydrogen forms with the elements polonium, chlorine, arsenic, and tin. element compound formula geometry polonium _________linearbenttrigonal pyramidaltetrahedral chlorine _________linearbenttrigonal pyramidaltetrahedral arsenic _________linearbenttrigonal pyramidaltetrahedral tin _________linearbenttrigonal pyramidaltetrahedral

Using the trend in the periodic table, and position of an element in it, the smallest element is

Using the trend in the periodic table, and position of an element in it, the smallest element is a. hydrogen b. Helium c. Oxygen d. Carbon

f.) Predict the products of oxidation and dehydration reactions of alcohol

f.) Predict the products of oxidation and dehydration reactions of alcohol g.) Describe the oxidation and reduction reactions of thiols to form or break disulfides h.) Predict the products of oxidation and reduction reactions of aldehydes and ketones i.) Describe the formation and hydrolysis of hemiacetals and acetals from alcohols and aldehydes or ketones

An element in the 4th row of the periodic table has the following ionization energies: i1...

An element in the 4th row of the periodic table has the following ionization energies: i1 = 762kJ/mol, i2 = 1021 kJ/mol, i3 = 1203 kJ/mol, i4 = 1402 kJ/mol, i5 = 5002 kJ/mol, i6 = 8321 kJ/mol, i7 = 10243 kJ/mol, i8 = 13210 kJ/mol What is the identity of the element?

Boron is the fifth element in the periodic table. For the first ionization of boron, the...

Boron is the fifth element in the periodic table. For the first ionization of boron, the ionization energy is 0.8006 MJ/mol. Calculate the effective nuclear charge (Zeff) for the first ionization of boron.

The element nitrogen is found in the second row of the periodic table and has an...

The element nitrogen is found in the second row of the periodic table and has an atomic number of 7. how many electrons must nitrogen gain in order for its valence shell to be full? The answer is 3 but what's the concept behind this?

The location of an element in the periodic table provides awealth of information about effective...

The location of an element in the periodic table provides a wealth of information about effective nuclear charge, size, ionization energy, and electron affinity. Using this information, it is possible to predict which elements are more likely to behave as oxidizing agents and which are more likely to behave as reducing agents. Use your knowledge of periodic trends to answer the following questions about the properties you would expect of an element that is a good reducing agent.a. Zeff :...

Assign an oxidation state to each element or ion: Part A V Express your answer as...

Assign an oxidation state to each element or ion: Part A V Express your answer as a signed integer. Part B Mg2+ Express your answer as a signed integer. Part C Cr3+ Assign an oxidation state to each atom in each polyatomic ion. Part B Express your answer as a signed integer. oxidation state of O: Part C OH− Express your answer as a signed integer. oxidation state of O: Part D Express your answer as a signed integer. oxidation...

Rank the following bonds from least polar to most polar: C-F Si-F Ga-F Predict the type...

Rank the following bonds from least polar to most polar: C-F Si-F Ga-F Predict the type of bond that would be formed between each of the following pairs of atoms: Ionic Polar Covalent Nonpolar Covalent K and Br Ionic Polar Covalent Nonpolar Covalent Cl and I Ionic Polar Covalent Nonpolar Covalent Li and N Ionic Polar Covalent Nonpolar Covalent C and H Classify the bonding in each compound: Ionic Nonpolar Covalent Polar Covalent HBr Ionic Nonpolar Covalent Polar Covalent Br2 Ionic Nonpolar Covalent Polar Covalent I2 Ionic...

Question