Q1 The model is useful for predicting molecular shape and estimating bond angles.
Q2 Lewis dot diagram, electron dot diagrams and electron dot stuctures are generally known as structures.
Q3 An SP hybrid orbital is formed by mixing together the 2S and atomic orbitals.
Q4 Hybridization Theory states that a covalent bond is formed by the of two singly atomic orbitals.
Q5 Hexaaquaaluminium means water molecules is wrapped around an aluminium ion.
Q6 Ions with water molecules attached are described as ions.
Q7 The fact that aluminium chloride sublimes at about$$\ 180^{o}$$ shows that bond exist between its molecule.
Q8 Aluminium chloride exist as a in the vapour state.
Q9 $$\{NH_{4}^{+}\}$$, are formed by the transfer of a $$\{H^{+}\}$$ from the hydrogen chloride to the pair of electrons on the $$\{NH_{3}\}$$.
Q10 A dative covalent bond is also called __bond.
Q11 Polythene,PVC, nylon, teflon, are all examples of __.
Q12 In diamond, carbon atoms are bonded to each other in directions.
Q13 Graphite can be used as a because each carbon atom slip over one another.
Q14 In graphite, one carbon-carbon bond out of the three carbons is a _.
Q15 In diamond, all the carbon atoms share one electron with each of their neighbouring atoms.
Q16 Graphite is the main component of the in pencils.
Q17 Carbon atoms are entirely bound together by bond to form diamond.
Q18 The molecular formular for isooctane is __.
Q19 Magnesium oxide has a melting point than sodium chloride.
Q20 Unlike covalent molecules, all ionic compounds are solids at room temperature.
Q21 The most abundant halogen is .
Q22 The 3p subshell in the ground state of atomic Xenon contains electrons.
Q23 is the energy required to convert a solid to a gas.
Q24 The subshell contains only one orbital.
Q25 is the energy required to convert a liquid to gas .
Q26 The lowest energy shell that contains f orbitals is the shell with n= _.
Q27 is the energy absorbed or released when an electron is added to a gaseous atom
Q28 is the energy required to remove one electron from a gaseous atom.
Q29 A co-ordinate bond is a covalent bond in which both electrons come from atom.
Q30 All ionic compounds are in water .
Q31 The law of conservation of energy is the same as the law of Thermodynamics.
Q32 The concept behind the Born-Haber cycle is based on law.
Q33 The energy of an ionic crystal is responsible for the formation and stability of ionic crystal structures.
Q34 Heat of formation is virtually for ionic compound.
Q35 Methane has a shape.
Q36 The second electron affinity numbers and beyond is always .
Q37 Lattice energies are always large numbers.
Q38 Bond energy is the energy required to break a covalent bond.
Q39 There are bond pairs around the central carbon atom in the Lewis structure of methane.
Q40 Heat of vaporization is the required to convert a liquid to a gas.
Q41 When more electrons are removed from an atom, the ionization energy .
Q42 Ionization energy is the energy required to remove one electron from a atom.
Q43 Heat of sublimation are always numbers.
Q44 Non-metals often form molecules.
Q45 All ionic compound adopts a similar dimensional structure.
Q46 The stable form of sodium chloride involves a very large number of NaCl units arranged in a millions of atoms across.
Q47 Elements in the first few columns of the periodic table have a few more electrons than predicted by the rule.
Q48 The halogens gains one electron to form ions.
Q49 Alkali metals loses one electron to form ions.
Q50 Charged species with each other.
Q51 Elements in group II and group VI form positive and negative ions respectively.
Q52 is formed when nuclei combine with electrons.
Q53 Molecules are made from __.
Q54 Sodium ion is than sodium atom.
Q55 Using Pauling scale in measuring electron affinity, the highest value assigned is .
Q56 It is impossible to measure the electronegativity of an atom
Q57 Element with low are said to be electropositive.
Q58 In the Group 2 elements , the filled 2s apparently shields the nucleus making electron affinities to be slightly endothermic
Q59 becomes more exothermic as we move from left to right across a period.
Q60 Electron affinities tends to be much smaller than energies.
Q61 ___________ is the energy absorbed or released when an ionic compound is made from its constituents elements.
Q62 The energy released when gaseous ions are converted into solid ionic compound is called _________.
Q63 _____________ is not a property of ionic compounds.
Q64 How many Lewis stuctures can be written for sulphur dioxide?
Q65 The valence bond theory states that ;________________.
Q66 All are the examples of molecules with dipole-dipole attraction except _______________.
Q67 Which of the following is not true of London forces?
Q68 A weak intermolecular force arising from quantum
induced instantaneous polarization multipoles in molecules describes
_____________.
Q69 A _________ is formed when a hydrogen atom on one water molecule is attracted to the oxygen of another water molecule.
Q70 Instantaneous dipole-induced dipole forces are known as _____________.
Q71 Metals are well known to be solids except for ______________.
Q72 The weak "bond" between the fluorine atom and the hydrogen atom is called ____________.
Q73 In which of the following does electrons move around easily?
Q74 Which of the following is not true of metals?
Q75 Aluminium chloride is covalent , but when it dissolves in water, ____________ are produced.
Q76 Ions with water molecules attached are described as ____________.
Q77 The reaction between ammonia and boron trifluoride demonstrates the formation of compound involving __________ bond.
Q78 The $$\{H_{3}O^{+}\}$$ ion is called ___________.
Q79 ______________ are formed by the transfer of a
hydrogen ion from hydrogen chloride to the lone pair of electrons on
ammonia molecule.
Q80 Whem ammonia and hydrogen chloride reacts, a thick ___________smoke of solid ammonium chloride is formed.
Q81 $$\{C_{9}H_{8}O_{4}\}$$ is the formular of a medicinal molecule called _______________.
Q82 $$\{C_{27}H_{46}O\}$$ is the molecular formular of _____________.
Q83 The compound with the formular $$\{C_{8}H_{18}\}$$ is called ____________.
Q84 One of the main components of petrol for cars is ______________.
Q85 When a shared pair of electrons come from the same atom, a _________ bond is formed.
Q86 A _________ bond is formed by two atoms sharing a pair of electrons.
Q87 The folowing are examples of polymers except ______________.
Q88 The letter H in the Schrodinger equation is called __________.
Q89 The more accurately the position of a particle
wave is known,the less accurately the momentum can be determined and
vice versa. This is a summary of which principle?
Q90 Electron __________ is an evidence for the wave nature of the electron.
Q91 What accounts for electrons spreading out rather than being located in one particular?
Q92 The value 6.62608 × 10^-34 Js is equal to __________in equation 1 above.
Q93 $$\lambda=\frac{h}{mv}$$ ---------equation 1. $$\lambda$$ in equation 1, represents __________.
Q94 The science which takes into account yhe dual nature of matter was developed independently by ____________.
Q95 The branch of science that deals with the dual behaviour of matter is called _________.
Q96 Which of these are the limitations of the Bohr's Theory?
Q97 Which of the following is the odd one out?
Q98 The Balmer series lies mostly in the __________ region of the spectrum.
Q99 The value of Rydberg's constant, R is _____________.
Q100 According to Coulomb's law, the force of attraction between the nucleus and the electron is __________.
Q101 The simplest spectrum is of _______________.
Q102 If there is a variation in the number of
electrons and number of protons in the nucleus of an atom, then the atom
is a /an________ .
Q103 The electrical charge on the neutron is ____________.
Q104 The mass of an electron is about _________ times smaller than that of the proton and neutron.
Q105 _____________ was the first to propose the basic structure of the atom.
Q106 Ionization energies increases with nuclear charge _________.
Q107 The addition of one or more electrons to an existing shell ____________ electron-electron repulsion.
Q108 Atomic radius increases _____________.
Q109 Atomic size decreases _____________.
Q110 ____________ is the effective radius of adjacent
atoms which are not chemically bonded in a solid but are presumably in
"contact".
Q111 ______________ is half the distance between nuclei in a metallic crystal.
Q112 Which group of elements have five valence electrons in their outermost shell?
Q113 Which is the odd one out?
Q114 Group IV and V metals can lose either the
electrons from the p subshell, or from both the s and p subshells, thus
attaining a ____________ configuration.
Q115 Atoms prefer to have a filled outermost shell because this is more __________________.
Q116 The outermost shell of an atom is known as ____________.
Q117 No two electrons in the same atom can have
identical values for all four of their quantum numbers. Which principle
is this?
Q118 ___________ specifies the orientation in space of an orbital of a given energy and shape.
Q119 Which of these quantum numbers specifies the energy of an electron and the size of the orbital?
Q120 A wave function for an electron in an atom is called an __________.