How does the of Ionization Enthalpy of alkaline earth metals vary in comparison to alkali metals

How does the of Ionization Enthalpy of alkaline earth metals vary in comparison to alkali metals 
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The alkaline earth metals have low ionization enthalpies due to fairly large size of the atoms. Since the atomic size increases down the group, their ionization enthalpy decreases The first ionisation enthalpies of the alkaline earth metals are higher than those of the corresponding Group 1 metals. This is due to their small size as compared to the corresponding alkali metals. It is interesting to note that the second ionisation enthalpies of the alkaline earth metals are smaller than those of the corresponding alkali metals.  
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How does the of Ionization Enthalpy of alkaline earth metals vary in comparison to alkali metals

Description : How does the of Ionization Enthalpy of alkaline earth metals vary in comparison to alkali metals

Last Answer : Ans The alkaline earth metals have low ionization enthalpies due to fairly large size of the atoms. Since the atomic size increases down the group, their ionization enthalpy decreases The first ... enthalpies of the alkaline earth metals are smaller than those of the corresponding alkali metals.

How does the of Hydration Enthalpy of alkaline earth metals vary & compare it with alkali metals

Description : How does the of Hydration Enthalpy of alkaline earth metals vary & compare it with alkali metals

Last Answer : Ans The hydration enthalpies of alkaline earth metal ions decrease with increase in ionic size down the group. Be2+> Mg2+ > Ca2+ > Sr2+ > Ba2+ The hydration enthalpies of alkaline earth metal ions ... MgCl2 and CaCl2 exist as MgCl2.6H2O and CaCl2· 6H2O while NaCl and KCl do not form such hydrates.

How does the of Hydration Enthalpy of alkaline earth metals vary & compare it with alkali metals

Description : How does the of Hydration Enthalpy of alkaline earth metals vary & compare it with alkali metals  

Last Answer : The hydration enthalpies of alkaline earth metal ions decrease with increase in ionic size down the group. Be2+> Mg2+ > Ca2+ > Sr2+ > Ba2+ The hydration enthalpies of alkaline earth metal ... and CaCl2 exist as MgCl2.6H2O and CaCl2· 6H2O while NaCl and KCl do not form such hydrates.  

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 ionization enthalpy varies in alkali metals

Description : How the ionization enthalpy varies in alkali metals 

Last Answer : Ionization enthalpy decrease down the group from Li to Cs. 

Give reason .the compounds of alkaline earth metals are less ionic than alkali metals

Description : Give reason .the compounds of alkaline earth metals are less ionic than alkali metals

Last Answer : Ans This is due to increased nuclear charge and smaller size.

Give reason .the compounds of alkaline earth metals are less ionic than alkali metals

Description : Give reason .the compounds of alkaline earth metals are less ionic than alkali metals

Last Answer : This is due to increased nuclear charge and smaller size. 

Define ionization enthalpy. Name the factors on which ionisation enthalpy depends? How does it vary down the group and across a period?

Description : Define ionization enthalpy. Name the factors on which ionisation enthalpy depends? How does it vary down the group and across a period?

Last Answer : Define ionization enthalpy. Name the factors on which ionisation enthalpy depends? How does it vary down the group and across a period?

What is the most active group of nonmetals noble gases alkaline earth halogens alkali metals?

Description : What is the most active group of nonmetals noble gases alkaline earth halogens alkali metals?

Last Answer : The most active metals are alkali metals.The most active nonmetals are halogens.

Who has the most active group of nonmetals noble gases alkaline earth halogens alkali metals?

Description : Who has the most active group of nonmetals noble gases alkaline earth halogens alkali metals?

Last Answer : Kevin

Electrometallurgical methods of metal extraction is normally used for those metals (A) Whose oxide/ore is not reduced by carbon (B) Which fall in the category of alkali & alkaline earth metals (C) Which stands higher in the electrochemical series of the metal (D) All (A), (B) & (C)

Description : Electrometallurgical methods of metal extraction is normally used for those metals (A) Whose oxide/ore is not reduced by carbon (B) Which fall in the category of alkali & alkaline earth metals (C) Which stands higher in the electrochemical series of the metal (D) All (A), (B) & (C)

Last Answer : (D) All (A), (B) & (C)

State as to why: (a) A solution of Na2CO3 is alkaline? (b)alkali metals are prepared by electrolysis of their fused chlorides ? (c)sodium is found to be more useful than potassium ?

Description : State as to why: (a) A solution of Na2CO3 is alkaline? (b)alkali metals are prepared by electrolysis of their fused chlorides ? (c)sodium is found to be more useful than potassium ?

Last Answer : Ans. (a) It undergoes hydrolysis to produce a strong base NaOH . (b) When the aq. Solution of any alkali metal is subjected to electrolysis ,H2 instead of the alkali metal is produced at the ... of sugars and amino acids into the cells. Thus, sodium is found to be more useful than potassium.

The elements in group 1A of the periodic table are called: w) halogens x) alkaline earths y) alkali metals z) rare earths

Description : The elements in group 1A of the periodic table are called: w) halogens x) alkaline earths y) alkali metals z) rare earths

Last Answer : ANSWER: Y -- ALKALI METALS

Give reasons : a. Alkali metals have low ionization energies.  b. Inert gases have exceptionally high ionization energies.

Description : Give reasons : a. Alkali metals have low ionization energies.  b. Inert gases have exceptionally high ionization energies.

Last Answer : Give reasons : a. Alkali metals have low ionization energies. b. Inert gases have ... d. Noble gases possess relatively large atomic size.

Why second ionization energy of alkali metals are higher than first ionization energy?

Description : Why second ionization energy of alkali metals are higher than first ionization energy?

Last Answer : The attraction between the electrons involved and the atomic nucleus is stronger.

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)

Within a given period of the periodic table, the element with the lowest ionization energy is: w) transition metal x) alkali metal y) halogen z) noble gas

Description : Within a given period of the periodic table, the element with the lowest ionization energy is: w) transition metal x) alkali metal y) halogen z) noble gas

Last Answer : ANSWER: X -- ALKALI METAL

The order of Ionization enthalpy between following atoms is?

Description : The order of Ionization enthalpy between following atoms is?

Last Answer : B, Tl, Ga, Al and In. Ans.B>Tl>Ga> Al> In.

From each set, choose the element with largest ionization enthalpy and explain your answer. (a) F, O, N (b) Mg, P, Ar (c) B, Al, Ga

Description : From each set, choose the element with largest ionization enthalpy and explain your answer. (a) F, O, N (b) Mg, P, Ar (c) B, Al, Ga

Last Answer : Ans. (a). The element fluorine F has the largest ionization enthalpy because in general, it increases along the period. These elements belong to the second period in the order is: N, O, F. Therefore, ... the order of B, Al, Ga. Therefore, the first element B is expected to have the largest value.

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

(a). Which is largest in size- Cu+ , Cu+2, Cu and why? (b). which element in the periodic table has the highest ionization enthalpy? (c). Which element is more metallic in the periodic table.?

Description : (a). Which is largest in size- Cu+ , Cu+2, Cu and why? (b). which element in the periodic table has the highest ionization enthalpy? (c). Which element is more metallic in the periodic table.?

Last Answer : Ans. (a). Cu is largest due to less effective nuclear charge. It has 29 electrons, 29 protons, Cu+ has 28 electrons and 29 protons, Cu2+ has 27 electrons and 29 protons. (b). He has highest ionization enthalpy. (c). Mg is more metallic due to lower ionization energy

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.

Why the ionization enthalpy decreases down the group ?

Description : Why the ionization enthalpy decreases down the group ? 

Last Answer : This is because, the Increase in atomic size is more predominant over increasing nuclear charge and the outer most electrons are very well screened from the nuclear charge by the inner shell electrons 

Which group elements show very low ionization enthalpy in the periodic table?

Description : Which group elements show very low ionization enthalpy in the periodic table?

Last Answer : First group elements (alkali metals) 

Give reason for the higher melting point and boiling point of alkali earth metals than alkali metals.

Description : Give reason for the higher melting point and boiling point of alkali earth metals than alkali metals. 

Last Answer : The melting and boiling points of these metals are higher than the corresponding alkali metals due to smaller sizes. 

When talking about the periodic table, what are the trends of precipitates as you move down the column of alkaline earth metals?

Description : When talking about the periodic table, what are the trends of precipitates as you move down the column of alkaline earth metals?

Last Answer : Homework, eh? :)

What are the uses of alkaline earth metals ?

Description : What are the uses of alkaline earth metals ?

Last Answer : Beryllium is used in the manufacture of alloys. Copper-beryllium alloys are used in the preparation of high strength springs. Metallic beryllium is used for making windows of X-ray tubes. Magnesium ... vacuum tubes. Radium salts are used in radiotherapy, for example, in the treatment of cancer.

Why II group elements are called alkaline earth metals ?

Description : Why II group elements are called alkaline earth metals ? 

Last Answer :  These are called so because their oxides and hydroxides are alkaline in nature and these metal oxides are found in the earth’s crust.  

Which alkali metal will have highest hydration enthalpy ?

Description : Which alkali metal will have highest hydration enthalpy ?

Last Answer : Ans. Li

Why alkali metal have low ionization energy?

Description : Why alkali metal have low ionization energy?

Last Answer : Ionization energy is the energy required to remove an electronfrom an atom or ion. Low ionization energy indicates that it takesless energy to remove an electron from the atom. The alkali ... are more and more electrons in theoutermost energy level, requiring more energy to remove anelectron.

Why alkali metal have low ionization energy?

Description : Why alkali metal have low ionization energy?

Last Answer : Ionization energy is the energy required to remove an electronfrom an atom or ion. Low ionization energy indicates that it takesless energy to remove an electron from the atom. The alkali ... are more and more electrons in theoutermost energy level, requiring more energy to remove anelectron.

Which element from the following pairs has higher ionization enthalpy? B and TI, N and Bi

Description : Which element from the following pairs has higher ionization enthalpy? B and TI, N and Bi

Last Answer : Which element from the following pairs has higher ionization enthalpy? B and TI, N and Bi

a. Which atom should have smaller ionization enthalpy, oxygen or sulfur? b. The lithium forms +1 ions while berylium forms +2 ions ?

Description : a. Which atom should have smaller ionization enthalpy, oxygen or sulfur? b. The lithium forms +1 ions while berylium forms +2 ions ?

Last Answer : With the help of diagram answer the questions given below : a. Which atom should have smaller ... forms +1 ions while berylium forms +2 ions ?

Ionization enthalpy of Li is 520 kJ mol^(-1) while that of F is 1681 kJ mol^(-1) . Explain.

Description : Ionization enthalpy of Li is 520 kJ mol^(-1) while that of F is 1681 kJ mol^(-1) . Explain.

Last Answer : Ionization enthalpy of Li is 520 kJ mol-1 while that of F is 1681 kJ mol-1. Explain.

Why the second ionization enthalpy is greater than the first ionization enthalpy ?

Description : Why the second ionization enthalpy is greater than the first ionization enthalpy ?

Last Answer : Why the second ionization enthalpy is greater than the first ionization enthalpy ?

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

Alkaline earth metals have low values of electronegativity; which decrease down the group.

Description : Alkaline earth metals have low values of electronegativity; which decrease down the group.

Last Answer : Explain : Alkaline earth metals have low values of electronegativity; which decrease down the group.

Which group of elements is called alkaline earth metals ?

Description : Which group of elements is called alkaline earth metals ?

Last Answer : 1st A group because the oxides and hydrides are alkaline in nature Among 1A group elements why the element lithium is the most powerful, reducing agent in equivalent state Due to its low sublimation and hydration energy

What is an alkaline alkali ?

Last Answer : According to the Bronsted-Laurie theory, when an acid reacts with an alkali , the acid forms its binding alkali and the alkali binds its binding acid by exchanging a proton (hydrogen cation or H +) .

What are the alkali metals ?

Description : What are the alkali metals ?

Last Answer : The remaining 6 elements of hydrogen in group 1 of the periodic table .

Give reason for the following: (i)alkali metals do not occur free in nature. (ii)alkali metals have low I .E. (iii)LiI is more soluble than KI in ethanol.

Description : Give reason for the following: (i)alkali metals do not occur free in nature. (ii)alkali metals have low I .E. (iii)LiI is more soluble than KI in ethanol.

Last Answer : Ans.(i)They are highly reactive in natur (ii) Because of large atomic size. (III)LiI is more covalent in character than KI

why alkali metals impart color to the flame?

Description : why alkali metals impart color to the flame?

Last Answer : Ans. Alkali metals have low ionization enththalpies. Their valence electrons get excited by absorbing energy from the flame. When these electrons return to the ground state, the energy is emitted In the form of light.

what are the common physical features of alkali metals?

Description : what are the common physical features of alkali metals?

Last Answer : Ans. Large Atomic and ionic radii, Low ionization enthalpies, metallic character, low melting and boiling Point, form ionic bond, low density,show flame coloration ,photoelectric effect.

what do you understand by “Non stoichiometric hydrides”? Do you think this type of hydrides to be formed by alkali metals? Justify your answer.

Description : what do you understand by “Non stoichiometric hydrides”? Do you think this type of hydrides to be formed by alkali metals? Justify your answer.

Last Answer : Ans: Hydrides which are deficient in hydrogen and in which the ratio of hydrogen to metal is fractional are called non-stoichiometric hydrides. This type of hydrides are formed by d-and ... they form only stoichiometric hydrides. In other words alkali metals do not form non-stoichiometric hydrides.

Which one of the alkali metals, forms only, the normal oxide, M2O on heating in air (1) Na (2) Rb (3) K (4) Li

Description : Which one of the alkali metals, forms only, the normal oxide, M2O on heating in air (1) Na (2) Rb (3) K (4) Li

Last Answer : Li

Mention the Points of Difference between ‘Lithium and other Alkali Metals’

Description : Mention the Points of Difference between ‘Lithium and other Alkali Metals’

Last Answer : (i) Lithium is much harder. Its m.p. and b.p. are higher than the other alkali metals. (ii) Lithium is least reactive but the strongest reducing agent among all the alkali metals. ... and Li2O are comparatively much less soluble in water than the corresponding compounds of other alkali metals. 

Explain the stability of carbonates & bicarbonates of alkali metals .

Description : Explain the stability of carbonates & bicarbonates of alkali metals . 

Last Answer : The alkali metals form salts with all the oxo-acids. They are generally soluble in water and thermally stable. Their carbonates (M2CO3) and in most cases the hydrogencarbonates (MHCO3) also are highly ... the formation of more stable Li2O and CO2. Its hydrogencarbonate does not exist as a solid.