AP SSC 10th Class Physical Science Chapter 10 Solution – Chemical Bonding
Andhra Pradesh SSC 10th Class Physical Science Chapter 10 Chemical Bonding Solution for AP SSC 10th Class Physics/Chemistry Exam. Lots of Students of Andhra Pradesh Board will search on internet for Andhra Pradesh Class 10 Physical Science Textbook Solution or Study Material for AP SSC 10th exam. Here you search will end! Here in this page we have provided for all question answer for Chapter 10 Chemical Bonding.
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AP 10th Class Physics Chapter 10 Chemical Bonding Solution
(1) List the factors that determine the type of bond that will be formed between two atoms?(AS1)
Ans: –The factor that effect the bond between two atoms are ionization energy, electronegativity, electron affinity and the state of the atoms.
(2) Explain the difference between the valence electrons and the covalence of an element.(AS1)
Ans: –Covalency means how many bonds are made using the last orbital whereas valence electron are how many electron of that atoms used to form bond.
(3) A chemical compound has the following Lewis notation: (AS1)
(a) How many valence electrons does element Y have?
(b) What is the valency of element Y?
(c) What is the valency of element X?
(d) How many covalent bonds are there in the molecule?
(e) Suggest a name for the elements X and Y. (AS2)
Ans :- (a) Y have 6 valence electron.
(b) Valency of the element y is 2.
(c) Valency of x is 1.
(d) There are 2 covalent bonds in the molecule.
(e) X probably be H2 and y may be O2.
(4) What do only valence electrons involve in bond formation? Why not electron of inner shells? Explain. (AS1)
Ans: –The electron of the inner shell could not form bonds because it strongly attached by nucleus. Whereas valence electron are loosely attached to in inner nucleus so it more active in nature. For this advantage valence electron from bond.
(5) Explain the formation of sodium chloride and calcium oxide on the basis of the concept of electron transfer from one atom to another atom. (AS1)
Ans: –From electronic configuration of Na and Ca we see that there are valence electron in Na 3s^1 and Ca 3p^5. So Na become octet by losing its valence electron and Ca need to fill up its octet by receiving that electron.
(6) A, B, and C are three elements with atomic number 6, 11 and 17 respectively.
(i) Which of these cannot form ionic bond? Why? (AS1)
(ii) Which of these cannot form covalent bond? Why? (AS1)
(iii) Which of these can form ionic as well as covalent bonds? (AS1)
Ans: –The compound that 6, 11, and 17 atomic number are C, Na, and Cl.
(i) As in carbon atom there is no free electron so it doesn’t form ionic bond and it only share its electron to form covalent bond.
(ii) Na will try to lose its electron present in 3s^1 orbital to become octet so it only form ionic form not covalent bond.
(ii) The element Cl will form both ionic and covalent bond. It will form ionic bond with help of the electron present on 3p^5 orbital. To HCl it form covalent bond by sharing it electron.
(7) How bond energies and bond lengths of molecule helps us in predicting their chemical properties? Explain with examples. (AS1)
Ans: –If the bond length in two atom is large then the energy required to break it will be easier whereas the bond length if small then more energy required to break it. For example in I2 the bond energy required less as it has more bond length.
(8) Predict the reasons for low melting point for covalent compounds when compared with ionic compound. (AS2)
Ans: –The covalent compound have week Vander Waal’s bond so its melting point is low. But the bond of ionic compound has more strong compare to covalent bond. So the energy should be high to break the bond.
(10) Draw simple diagrams to show how electrons are arranged in the following covalentmolecules:(AS5)
(a) Calcium oxide (CaO)
(b) Water (H2O)
(c) Chlorine (Cl2)
Ans:-
(11) Represent the molecule H2O using Lewis notation. (AS5)
Ans: –
(12) Represent each of the following atoms using Lewis notation: (AS5)
(a) beryllium
(b) calcium
(c) lithium
Ans:-
(a) Lewis notation of Be is Be: (1s^22s^2).
(b) Lewis notation of Ca is Ca: (1s^22s^22p^63s^23p64s^2).
(c)Lewis notation of Li is Li. (1s^22s^1).
(13) Represent each of the following molecules using Lewis notation: (AS5)
(a) bromine gas (Br2)
(b) calcium chloride (CaCl2)
(c) carbon dioxide (CO2)
Ans: –
(14) Two chemical reactions are described below. (AS5)
- Nitrogen and hydrogen react to form ammonia (NH3)
- Carbon and hydrogen bond to form a molecule of methane (CH4).
For each reaction, give:
(a) The valency of each of the atoms involved in the reaction. (AS1)
(b) The Lewis structure of the product that is formed. (AS5)
Ans: –In the first reaction the valency of N2 is 3 and H2 is 1.In the second reaction the valency of carbon is 4 and hydrogen is 1.
(b)
(15) How Lewis dot structure helps in understanding bond formation between atoms? (AS6)
Ans: –The outer most shell of any atom are represent through dot structure by lewis notation. As the outer most shell is represented by dot structure we can easily understand the valency of any atom which tells us about bond reaction of that atom.
(16) What is octet rule? How do you appreciate role of the ‘octet rule’ in explaining the chemical properties of elements? (AS6)
Ans: –The outer most shell of any atom tends to fill with 8 electron, this tendency of the atom called octet rule. For this octet rule any atom always try to fill up their outer most shell by loosing or gaining electron. The atom which has less that 4 electron in their outer shell try to octet by losing electron whereas the atom which has more than 4 atom in their outermost shell try to fill octet by gaining the electron.
(17) Explain the formation of the following molecules using valence bond theory
(a) N2 molecule
(b) O2 molecule.
Ans:-
(18) What is hybridization? Explain the formation of the following molecules using hybridization
(a) Be Cl2
(b) BF3
Ans: –When the atom mixed with another atom orbital to form a new orbital is known as hybridization. Although the new orbital form the electron must be same in that.
FILL IN THE BLANKS
(1) Electrons in…..outermost……. shell are called valence electrons.
(2) Except …….helium…… gas all other noble gases have octet in their valence shell.
(3) Covalency of elements explains about member of…..covalent bond……….. formed by the atom.
(4) Valence bond theory was proposed by ….Linus Pauling and John C Slater………
(5) In ………covalent …………bonding the valence electrons are shared among all the atoms of themetallic elements.
MULTIPLE CHOICE QUESTIONS
(1) Which of the following elements is electronegative? –
(b) Oxygen.
(2) An element 11X23 forms an ionic compound with another element ‘Y’. Then the charge on the ion formed by X is –
(a) +1.
(3) An element ‘A’ forms a chloride ACl4. The number electrons in the valence shell of ‘A’–
(d) 4.
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