Define the following : Atomic Radii , Ionization Energy , Electron Affinity , Electronegativity.

Define the following : Atomic Radii , Ionization Energy , Electron Affinity , Electronegativity.
by

1 Answer

Answer :

Ans :(1) Atomic Radii :
“An atom does not have strictly defined boundaries so it is impossible to determine the exact radius of an atom but theoretically it is defined as half the distance between the two adjacent nuclei of two similar atoms in touch with each other”.
Unit :
It is measured in Angstrom. 1A0 = 10-8 cm.
Trend in Group :
It increases from top to bottom due to increase in number of shells.
Trend in Period :
It decreases from left to right due to increase in nuclear charge.
(2) Ionization Energy :
“The minimum amount of energy required to remove the most loosely bound electron from the valence shell of a gaseous atom or ion in ground state to form a positive ion (cation) is called first ionization energy or ionization potential”.
Unit :
It is measured in K.Jole / Mole or (ev) electron volt per atom. It depends upon the atomic size & nuclear charge.
Trend in Group :
It decreases from top to bottom due to increase in number of shells.
Trend in Period :
It increases from left to right due to decrease in atomic size & increase in nuclear charge.
(3) Electron Affinity :
“The energy change that occurs when an electron is gained by an atom in the gaseous state is called Electron Affinity. Electron Affinity for the addition of first electron is negative but for further addition of electrons it is positive.”
Unit :
It is measured in K.Jole / Mole or (ev) electron volt per atom. It depends upon the atomic size & nuclear charge.
Trend in Group :
It decreases from top to bottom due to increase in number of shells in atom which decreases its force of attraction.
Trend in Period :
It increases from left to right in a period due to increase in nuclear charge.
(4) Electronegativity :
“The relative tendency of an atom in a molecule to attract the shared pair of electron towards itself is called Electronegativity.”
Unit :
It is denoted by a number & has no unit.
Trend in Group :
It decreases from top to bottom due to increase in number of shells in atom which decreases its force of attraction.
Trend in Period :
It increases from left to right in a period due to increase in nuclear charge.
by

Related questions

The energy released when an extra electron is added to a neutral gaseous atom is called (a) Bond energy (b) Electron affinity (c) Ionization potential (d) Electronegativity

Description : The energy released when an extra electron is added to a neutral gaseous atom is called (a) Bond energy (b) Electron affinity (c) Ionization potential (d) Electronegativity

Last Answer : Ans:(b)

Explain the trend of the following in group 13 elements : A. atomic radii  B. ionization enthalpy  C. electron affinity

Description : Explain the trend of the following in group 13 elements : A. atomic radii  B. ionization enthalpy  C. electron affinity

Last Answer : Explain the trend of the following in group 13 elements : A. atomic radii B. ionization enthalpy C. electron affinity

AS A GROUP, the halogens have the largest: w) atomic radii x) Boiling points y) electronegativities z) ionization energies

Description : AS A GROUP, the halogens have the largest: w) atomic radii x) Boiling points y) electronegativities z) ionization energies

Last Answer : ANSWER: Y -- ELECTRONEGATIVITIES

Which among the following is not a characteristic of transition metals? (1) Tendency to gain electrons (2) Low electronegativity (3) Low ionization energy (4) Malleability

Description : Which among the following is not a characteristic of transition metals? (1) Tendency to gain electrons (2) Low electronegativity (3) Low ionization energy (4) Malleability

Last Answer : (1) Tendency to gain electrons Explanation: The transition metals have a tendency to lose electrons. Since the electrons in the highest energy level are actually on a lower principal enemy number than the ... ions, the 4s electrons are always lost first; so, they form only cations (positive ions).

Which among the following is not a characteristic of transition metals? (1) Tendency to gain electrons (2) Low electronegativity (3) Low ionization energy (4) Malleability

Description : Which among the following is not a characteristic of transition metals? (1) Tendency to gain electrons (2) Low electronegativity (3) Low ionization energy (4) Malleability 

Last Answer : Tendency to gain electrons

How IS The electronegativity trend relates to the first ionization energy trend?

Description : How IS The electronegativity trend relates to the first ionization energy trend?

Last Answer : Electronegativity and first ionization energy both increasegoing up the Periodic Table.

Which of the following terms refers to the energy released when an electron is added to a neutral atom? w) electrovalence x) electron affinity y) electroconductance z) none of these

Description : Which of the following terms refers to the energy released when an electron is added to a neutral atom? w) electrovalence x) electron affinity y) electroconductance z) none of these

Last Answer : ANSWER: X -- ELECTRON AFFINITY

Which of the following properties is not true for an alkali metal? (a) Low electronegativity (b) Low ionisation energy (c) Low atomic volume (d) Low density

Description : Which of the following properties is not true for an alkali metal? (a) Low electronegativity (b) Low ionisation energy (c) Low atomic volume (d) Low density

Last Answer : Ans:(c)

As one goes across a period in the periodic table, the ionization energy generally increases for one of the following reasons. Is it because of the increasing w) atomic radius x) melting point y) nuclear charge z) density

Description : As one goes across a period in the periodic table, the ionization energy generally increases for one of the following reasons. Is it because of the increasing w) atomic radius x) melting point y) nuclear charge z) density

Last Answer : ANSWER: Y -- NUCLEAR CHARGE

Heavy metals got their name because compared to other atoms they have - (1) Higher densities (2) Higher atomic masses (3) Higher atomic numbers (4) Higher atomic radii

Description : Heavy metals got their name because compared to other atoms they have - (1) Higher densities (2) Higher atomic masses (3) Higher atomic numbers (4) Higher atomic radii

Last Answer : (2) Higher atomic masses Explanation: Arsenic, beryllium, cadmium, chromium, lead, manganese, mercury, nickel, and selenium are some of the metals called 'heavy' because of their high relative atomic ... and can cause damage or death in animals, humans, and plants even at very low concentrations.

How does the atomic and Ionic Radii of alkaline earth metals vary in comparison to alkali metals

Description : How does the atomic and Ionic Radii of alkaline earth metals vary in comparison to alkali metals

Last Answer : Ans The atomic and ionic radii of the alkaline earth metals are smaller than those of the corresponding alkali metals in the same periods. This is due to the increased nuclear charge in these elements. Within the group, the atomic and ionic radii increase with increase in atomic number.

How does the atomic and Ionic Radii of alkaline earth metals vary in comparison to alkali metals

Description : How does the atomic and Ionic Radii of alkaline earth metals vary in comparison to alkali metals 

Last Answer : The atomic and ionic radii of the alkaline earth metals are smaller than those of the corresponding alkali metals in the same periods. This is due to the increased nuclear charge in these elements. Within the group, the atomic and ionic radii increase with increase in atomic number.

How the atomic and ionic radii varies in alkali metals

Description : How the atomic and ionic radii varies in alkali metals 

Last Answer : The atomic and ionic radii of alkali metals increase on moving down the group i.e., they increase in size while going from Li to Cs.

What is the number of atomic radii along the face diagonal of a face-centered unit cell?

Description : What is the number of atomic radii along the face diagonal of a face-centered unit cell?

Last Answer : ANSWER: 4 

Heavy metals got their name because compared to other atoms they have (1) Higher densities (2) Higher atomic masses (3) Higher atomic numbers (4) Higher atomic radii

Description : Heavy metals got their name because compared to other atoms they have (1) Higher densities (2) Higher atomic masses (3) Higher atomic numbers (4) Higher atomic radii

Last Answer : Higher atomic masses

Evidence for the existence of energy level in atom is supplied by (a) Atomic numbers (b) Atomic radii (c) Spectral lines (d) Mass defects

Description : Evidence for the existence of energy level in atom is supplied by (a) Atomic numbers (b) Atomic radii (c) Spectral lines (d) Mass defects

Last Answer : Ans:(c)

Explain :  Electronegativity and electron gain enthalpy. Which of the two can be measured experimentally?

Description : Explain :  Electronegativity and electron gain enthalpy. Which of the two can be measured experimentally?

Last Answer : Explain : Electronegativity and electron gain enthalpy. Which of the two can be measured experimentally?

From the elements: Cl, Br, F, O, Al, C, Li, Cs and Xe; choose the following: (a) The element with highest negative electron gain enthalpy. (b) The element with lowest ionization enthalpy. (c) The element with smallest ionic radius. (d) The element with six electrons in the valence shell. (e) The element which is a liquid at room temperature. (f)The element which belongs to zero group. (g) The elements which forms largest number of compounds.

Description : From the elements: Cl, Br, F, O, Al, C, Li, Cs and Xe; choose the following: (a) The element with highest negative electron gain enthalpy. (b) The element with lowest ionization enthalpy. ( ... . (f)The element which belongs to zero group. (g) The elements which forms largest number of compounds.

Last Answer : Ans. (a). The element chlorine (Cl) has the highest negative electron gain enthalpy. (b). The element cesium (Cs) has lowest ionization enthalpy. (c). The element fluorine F has lowest atomic radius. (d ... zero group (or group 18). (g). The element carbon (C) forms the largest number of compounds.

Arrange the following order of the property indicated: (a). F, Cl, Br and I (negative electron gain enthalpy) (b). Mg, Al, Si and Na (ionization enthalpy) (c). C, N, O and F (second ionization enthalpy)

Description : Arrange the following order of the property indicated: (a). F, Cl, Br and I (negative electron gain enthalpy) (b). Mg, Al, Si and Na (ionization enthalpy) (c). C, N, O and F (second ionization enthalpy)

Last Answer : Ans. (a). I

Electron affinity of noble gases is - (1) zero (2) Low (3) High (4) Very high

Description : Electron affinity of noble gases is - (1) zero (2) Low (3) High (4) Very high

Last Answer : (1) zero Explanation: Most elements 'want' to have a complete electron shell with 8 electrons. Since the Noble Gases already have that 'perfect status' then they have an affinity of 0.

List the following atoms in order of increasing electron affinity: oxygen, boron, and fluorine.

Description : List the following atoms in order of increasing electron affinity: oxygen, boron, and fluorine.

Last Answer : ANSWER: (1) BORON, (2) OXYGEN, (3) FLUORINE

What electron would have the highest ionization energy for an oxygen atom?

Description : What electron would have the highest ionization energy for an oxygen atom?

Last Answer : What is the answer ?

The alkali metals have (a) Low ionization energy (b) High electronegativities (c) High m.p. (d) Electron configuration of ns2np1

Description : The alkali metals have (a) Low ionization energy (b) High electronegativities (c) High m.p. (d) Electron configuration of ns2np1

Last Answer : Ans:(a)

The energy required to completely remove an electron from the first Bohr orbit is called a) excited energy b) ionization energy c) accelerated energy d) orbital energy

Description : The energy required to completely remove an electron from the first Bohr orbit is called a) excited energy b) ionization energy c) accelerated energy d) orbital energy

Last Answer : b) ionization energy

The two elements required to form substitutional solid solution should not have (A) Same crystalline structure (B) Same valency (C) Widely differing electronegativity (D) Same atomic sizes

Description : The two elements required to form substitutional solid solution should not have (A) Same crystalline structure (B) Same valency (C) Widely differing electronegativity (D) Same atomic sizes

Last Answer : C) Widely differing electronegativity

Among the elements of the 3rd period from Na to Ar, pick out the element: (L-2) (a). with highest first ionization enthalpy. (b). with largest atomic radius. (c). that is most reactive non-metal. (d). that is most reactive metal.

Description : Among the elements of the 3rd period from Na to Ar, pick out the element: (L-2) (a). with highest first ionization enthalpy. (b). with largest atomic radius. (c). that is most reactive non-metal. (d). that is most reactive metal.

Last Answer : (a). Ar has highest first ionization enthalpy. (b). Na has large atomic radius (covalent radius). (c). Cl is more reactive non-metal in 3rd period. (d). Na is most reactive metal in third period.

1The elements of the second period of the Periodic Table are given below: Li Be B C N O F (a) Give reason to explain why atomic radii decrease from Li to F. (b) Identify the most (i) metallic and (ii)non-metallic element. -Science

Description : 1The elements of the second period of the Periodic Table are given below: Li Be B C N O F (a) Give reason to explain why atomic radii decrease from Li to F. (b) Identify the most (i) metallic and (ii)non-metallic element. -Science

Last Answer : a) It is because nuclear charge increases due to increase in atomic number, therefore, force of attraction between nucleus and valence electrons increases, i.e. effective nuclear charge increases, hence ... element is ‘F’ because it can gain electrons easily due to smallest atomic size.

The order of increasing size of atomic radii among the elements O,S,Se and As

Description : The order of increasing size of atomic radii among the elements O,S,Se and As

Last Answer : The order of increasing size of atomic radii among the elements O,S,Se and As A. `AsltSltOltSe` B. `SeltSltAsltO` C. `OltSltAsltSe` D. `OltSltSeltAs`

What group appears to have members of the largest atomic radii for a given period?

Description : What group appears to have members of the largest atomic radii for a given period?

Last Answer : This is the group 1.

Which element has the lowest electron affinity? -Do You Know?

Description : Which element has the lowest electron affinity? -Do You Know?

Last Answer : answer:

Assertion :- First electrons affinity fo all element is positive. Reason :- Successive electron affinity of all elements is negative

Description : Assertion :- First electrons affinity fo all element is positive. Reason :- Successive electron affinity of all elements is negative

Last Answer : Assertion :- First electrons affinity fo all element is positive. Reason :- Successive electron affinity ... D. If both Assertion & Reason are false

Electron affinity order of chalcogens is

Description : Electron affinity order of chalcogens is

Last Answer : Electron affinity order of chalcogens is A. `SgtSegtTegtO` B. `OgtSgtSegtTegtPo` C. `SgtOgtSegtTegtPo` D. `PgtPogtTegtSegtS`

Who can help me with this problem Rank the following elements by electron affinity from most positive to most negative I have the elements Ar Cl O Sb and Rb?

Description : Who can help me with this problem Rank the following elements by electron affinity from most positive to most negative I have the elements Ar Cl O Sb and Rb?

Last Answer : The order is: O, Cl, Sb, Rb, Ar.

The electron affinity for the inert gases is (a) Zero (b) High (c) Negative (d) Positive

Description : The electron affinity for the inert gases is (a) Zero (b) High (c) Negative (d) Positive

Last Answer : Ans:(a)

Which element has the lowest electron affinity?

Description : Which element has the lowest electron affinity?

Last Answer : Argon

Give reason: sodium has lower electron affinity than chlorine atom.

Description : Give reason: sodium has lower electron affinity than chlorine atom.

Last Answer : As electron affinity increases across a period (from left to right)

Which element has the lowest electron affinity?

Description : Which element has the lowest electron affinity?

Last Answer : Argon

Define : a. Ionic radius b. Electronegativity

Description : Define : a. Ionic radius b. Electronegativity

Last Answer : Define : a. Ionic radius b. Electronegativity

What is Electronegativity ?

Description : What is Electronegativity ?

Last Answer : : The ability of an electron pair to attract a shared electron pair is called the electron negativity of the element.

In general, as you move across a period (left to right) electronegativity: w) increases x) decreases y) remains the same z) increases or decreases

Description : In general, as you move across a period (left to right) electronegativity: w) increases x) decreases y) remains the same z) increases or decreases

Last Answer : ANSWER: W -- INCREASES

Which of the following elements has the highest electronegativity? w) Lithium x) Iodine y) Cesium z) Oxygen

Description : Which of the following elements has the highest electronegativity? w) Lithium x) Iodine y) Cesium z) Oxygen

Last Answer : ANSWER: D -- OXYGEN

The ionisation energy of dioxygen (`O_2`) is very close to that of Xenon. Also F and O have the highest electronegativity and consequently can oxidise

Description : The ionisation energy of dioxygen (`O_2`) is very close to that of Xenon. Also F and O have the highest electronegativity and consequently can oxidise

Last Answer : The ionisation energy of dioxygen (`O_2`) is very close to that of Xenon. Also F and O have ... (D) clathrates with He and Ne are highly expolsive.

The ionisation energy of dioxygen (`O_2`) is very close to that of Xenon. Also F and O have the highest electronegativity and consequently can oxidise

Description : The ionisation energy of dioxygen (`O_2`) is very close to that of Xenon. Also F and O have the highest electronegativity and consequently can oxidise

Last Answer : The ionisation energy of dioxygen (`O_2`) is very close to that of Xenon. Also F and O have ... +6HF underset(Delta)overset("475 K")to XeF_6+3H_2O`

The ionisation energy of dioxygen (`O_2`) is very close to that of Xenon. Also F and O have the highest electronegativity and consequently can oxidise

Description : The ionisation energy of dioxygen (`O_2`) is very close to that of Xenon. Also F and O have the highest electronegativity and consequently can oxidise

Last Answer : The ionisation energy of dioxygen (`O_2`) is very close to that of Xenon. Also F and O have the highest ... Ill), (lV) D. (D) (I), (lV)

What is ionization energy ?

Description : What is ionization energy ?

Last Answer : The amount of energy required to move the most loosely connected electrons from an isolated atom of an element to an infinite distance in a gaseous state is called the ionization energy of that element.

Why is the ionization energy of IA class elements lowest at any stage ?

Description : Why is the ionization energy of IA class elements lowest at any stage ?

Last Answer : Any phase of the Periodic Table starts with Group- IA on the left . At any stage, from left to right, the value of ionization potential gradually increases due to atomic size contraction. For this reason, the ionization energy of the elements of the leftmost IA group is the lowest.

What is the ionization energy of an element ?

Description : What is the ionization energy of an element ?

Last Answer : The amount of energy required to move the most loosely connected electrons from an isolated atom of an element to an infinite distance in a gaseous state is called the ionization energy of that element.

The element with highest first ionization energy is - (1) hydrogen (2) helium (3) lithium (4) sodium

Description : The element with highest first ionization energy is - (1) hydrogen (2) helium (3) lithium (4) sodium

Last Answer : (2) helium Explanation: The first ionisation energy is the energy required to remove the most loosely held electron from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of ... ) of Hydrogen: around 1200: Helium: about 2500; Lithium: about 500; and Sodium: about 500.

Among Li, Na, K, Rb, Cs, the element with lowest ionization energy is________

Description : Among Li, Na, K, Rb, Cs, the element with lowest ionization energy is________

Last Answer : Ans. Cs has lowest ionization enthalpy.

In general, as you move down a family the ionization energy: w) increases x) decreases y) remains the same z) increases or decreases

Description : In general, as you move down a family the ionization energy: w) increases x) decreases y) remains the same z) increases or decreases

Last Answer : ANSWER: X -- DECREASES