Chemical Bonding MCQs with answers in chemistry tests

Chemical Bonding MCQ with Answers

Chemical bonding MCQ with answers are a major component of the Army, Navy, and Pakistan Air Force (PAF) initial academic exams. For students hoping to join the Navy Supply Branch, Navy Operation Branch, or PN Cadets, these chemical bonding multiple-choice questions (MCQs) offer a thorough understanding of the key ideas in chemical bonding. They are also very helpful for people taking the exams for the Navy Education Branch, Navy Weapon Engineering Branch, and Navy Ordnance Branch.

Candidates can improve their understanding of Chemical Bonding by learning the multiple-choice questions (MCQs) in this subject, which is frequently a crucial component of the mathematics exams administered in these academic evaluations.

Chemical Bonding MCQ (Part-1)

  • In an ionic bond, electrons _______________ from one atom to another. (moved)
  •  Ionic bonds are formed between atoms with a large difference _______________. (electronegativity)
  • A positive ion is called _______________, a negative ion is called _______________. (cation, anion)
  • The formation of an ionic bond leads to the formation of _______________. (crystal grid)
  • Ionic compounds have ___________ melting points and boiling points because of the strong electrostatic attraction between the ions. (high)
  • In an ionic compound, the sum of the charges on the cations and anions must be _______________. (zero)
  • The crystal lattice structure of an ionic compound is held together by _______________. (electrostatic forces)
  • Ionic compounds conduct electricity when ___________ because the ions are free to move. (molten or dissolved in water)
  • The smallest unit of an ionic compound is called a ___________. (formula unit)
  • The formula for sodium chloride, a common ionic compound, is ___________. (NaCl)
  •  In an ionic bond, the atom that gains electrons becomes charged _______________. (negative)
  • The chemical symbol for chloride ion is _______________. (Cl)
  • Ionic compounds are usually ___________ at room temperature. (fixed)
  • Ionic bonding occurs between _______________ and _______________ elements. (metal, non-metallic)

Chemical Bonding and Molecular Structure MCQs

Chemical bonding and molecular structure mcqs provide useful preparation material for those aspiring to enter the armed forces, such as GD Pilots in the PAF or Aeronautical Engineering in the PAF. These chemical bonding multiple-choice questions (MCQs) address the fundamentals of chemical bonding, which are important for technical topics as well as PAF Admin & Special Duty Branch and PAF Logistics Branch exams.

Candidates can improve their comprehension of chemical bonding concepts by studying these chemical bonding multiple-choice questions (MCQs). This will help them perform well on the academic exams given by the PAF.

Chemical Bonding MCQ (Part-2)

  • The strength of an ionic bond is affected by the _______________ of the ions and the _______________ between them. (charge, distance)
  • A covalent bond involves ________ electrons between atoms. (division)
  • In a covalent bond, electrons are shared between ________. (two atoms)
  • Covalent bonds form between ________ or ________ atoms. (non-metals)
  • A covalent bond in which electrons are shared equally is called a ________ covalent bond. (non-polar)
  • A covalent bond in which electrons are unequally shared is called a ________ covalent bond. (polar)
  • A Lewis structure represents the ________ of electrons in a covalent molecule. (arrangement)
  • The number of covalent bonds formed by an atom is determined by its ________. (valence electrons)
  • The sharing of one electron pair between two atoms forms a ________ bond. (single)
  • The sharing of two pairs of electrons between two atoms forms a ________ bond. (double)
  • The sharing of three pairs of electrons between two atoms forms a ________ bond. (triple)
  • The shape of a molecule is determined by the ________ of its bonded atoms. (geometry)
  • A molecule whose central atom is bonded to four other atoms and has no lone pairs has a ________ geometry. (dihedral)
  • A molecule with a central atom bonded to three other atoms and one lone pair has ____ geometry. (triangular pyramid)
  • A molecule with a central atom bonded to two other atoms and two lone pairs has a ________ geometry. (bent)
  • The strength of a covalent bond is affected by the ________ between the bonded atoms. (distance)
  • In Lewis dot structures, dots are used to represent ________. (valence electrons)
  • The Lewis dot structure of an element is determined by its ________. (group number)
  • The central atom of a Lewis dot structure is usually an atom of ________ composition. (least electronegative)
  • The octet rule states that atoms tend to gain, lose, or share electrons to achieve a ________ electron configuration. (stable/noble gas)
  • Hydrogen obeys the ________ rule and forms only one bond in Lewis dot structures. (duet)
  • The Lewis dot structure of oxygen (O) consists of ____ dots surrounding the symbol “O”. (6)

Chemical bonding MCQs

Chemical bonding MCQs are a crucial component of the Army’s esteemed Technical Cadet Course. The basic ideas of chemical bonding are covered in these multiple-choice questions (MCQs), which are crucial for those who want to become Army EME Officers and Education Officers.

Furthermore, because they offer a strong basis in chemical bonding ideas, these chemical bonding multiple-choice questions are helpful for civilians taking tests for all branches of the armed services. Candidates can improve their chances of passing the exams and get an advantage over others by becoming familiar with these multiple-choice questions.

Chemical Bonding MCQ (Part-3)

  • The Lewis dot structure of nitrogen (N) consists of ________ dots surrounding the symbol “N”. (5)
  • The Lewis dot structure of carbon (C) consists of ________ dots surrounding the symbol “C”. (4)
  • In Lewis dot structures, lone pairs of electrons are denoted by ________. (point pairs)
  • The Lewis dot structure of water (H2O) consists of ________ dots around the oxygen atom (O) and ________ dots around each hydrogen atom (H). (8, 2)
  • The Lewis dot structure of methane (CH4) consists of ________ dots around the carbon atom (C) and ________ dots around each hydrogen atom (H). (8, 2)
  • The Lewis dot structure of ammonia (NH3) consists of ________ dots around the nitrogen atom (N) and ________ dots around each hydrogen atom (H). (8, 2)
  • The Lewis dot structure of carbon dioxide (CO2) consists of ________ dots around the carbon atom (C) and ________ dots around each oxygen atom (O). (8, 4)
  • The Lewis dot structure of nitrogen dioxide (NO2) consists of ________ dots around the nitrogen atom (N) and ________ dots around each oxygen atom (O). (5, 6)
  • When designing Lewis dot structures, it is important to follow the ____ rule, according to which the formal charge of atoms must be as close to zero as possible. (octet)
  • Molecular geometry refers to the ________ arrangement of atoms in a molecule. (3D)
  • The shape of a molecule is determined by the ________ of its bonded atoms. (geometry)
  • VSEPR theory stands for ________ electron pair repulsion theory. (Valence Shell electron pair repulsion)
  • According to the VSEPR theory, electron pairs in the valence shell of an atom repel each other and try to keep ________ away from each other. (so far)
  •  A molecule with two bonded atoms that do not have lone pairs is in ________ geometry. (linear)
  •  A molecule in which the central atom is bonded to three other atoms instead of lone pairs has a ________ geometry. (triangular plane)
  • A molecule with a central atom bonded to two other atoms and one lone pair has ____ geometry. (bent)
  • A molecule whose central atom is bonded to four other atoms and has no lone pairs has a ________ geometry. (dihedral)
  • A molecule with a central atom bonded to three other atoms and one lone pair has ____ geometry. (trigonal pyramid)
  • A molecule with a central atom bonded to two other atoms and two lone pairs has a ________ geometry. (curve).
  • The molecular geometry of carbon dioxide (CO2) is ________. (linear)
  • The molecular geometry of methane (CH4) is ________. (dihedral)
  • The molecular geometry of water (H2O) is ________. (bent)

Chemical Bonding MCQ Questions

It is impossible to overestimate the significance of MCQs on Chemical Bonding in defense force exams. These chemical bonding MCQ questions are specifically made to meet the academic criteria of different branches of the Army, Navy, and PAF. They ensure that applicants are well-prepared for the exams of the Navy Education Branch, Navy Air Defence Branch, and PN Cadets by covering a wide range of chemical bonding themes.

Additionally, applicants can succeed in other areas that incorporate mathematical principles because to the transferable knowledge they acquire from these multiple-choice questions. Therefore, it is strongly advised that those aspiring to the defense force include these multiple-choice questions in their study regimen.

Chemical Bonding MCQ (Part-4)

  • The molecular geometry of ammonia (NH3) is ________. (triangular pyramid)
  • The molecular geometry of carbon tetrachloride (CCl4) is ________. (dihedral)
  • Hybridization is the ________ of atomic orbitals to form hybrid orbitals. (mixture)
  • The concept of hybridization helps explain the ________ and ________ of chemical bonds. (power, form)
  • Hybrid orbitals are formed by combining ________ orbitals. (atom)
  • Sp hybridization is due to mixing of ________ s orbital and ________ p orbital. (one, one)
  • Sp2 hybridization is due to mixing of ________ s-orbital and ________ p-orbital. (one, two)
  • Sp3 hybridization is the result of the mixing of ________ s orbitals and ________ p orbitals. (one, three)
  • In sp hybridization, the hybrid orbitals are oriented ________ relative to each other. (linear)
  • In sp2 hybridization, the hybrid orbitals are oriented in a ________ arrangement. (triangular plane)
  • In sp3 hybridization, the hybrid orbitals are oriented in a ________ arrangement. (dihedral)
  • Hybridization of carbon in methane (CH4) is ________. (sp3)
  • Hybridization of carbon in ethylene (C2H4) is ________. (sp2)
  • Hybridization of carbon in ethyne (C2H2) is ________. (sp)
  •  The hybridization of nitrogen in ammonia (NH3) is ________. (sp3)
  • The hybridization of oxygen in water (H2O) is ________. (sp3)
  • The hybridization of nitrogen in the nitrate ion (NO3) is ________. (sp2)
  • Intermolecular forces are the forces of attraction between ________ molecules. (next to)
  • The strength of intermolecular forces determines the ________ and ________ properties of substances. (physical, chemical)
  • The weaker intermolecular force is the ________ force. (diffusion)
  • Disorders arise from fluctuations in the ________ distribution of electrons. (temporary)
  • The strength of dispersion forces depends on the ________ of the molecules involved. (polarizability)
  • Polar molecules have additional intermolecular forces called ________ forces. (dipole-dipole)
  • Dipole-dipole forces exist between ________ molecules with permanent dipoles. (polar)
  • Hydrogen bonding is a special dipole-dipole interaction that occurs when hydrogen is bonded to a ________, ________ or ________ atom. (nitrogen, oxygen, fluorine)
  • Hydrogen bonding is stronger than normal dipole-dipole forces because of hydrogen’s high ________. (electronegativity)
  • The intermolecular force responsible for the surface tension of liquids is the ________ force. (uniform)

Objective Question Answers for Chemical Bonding MCQs

Objective question answers for chemical bonding are a great study tool for those getting ready for college entrance exams in the Army, Navy, or PAF. These multiple-choice questions (MCQs) address the fundamental ideas of chemical bonding and are made to satisfy the academic requirements needed to be considered for admission to different branches of the armed forces.

Those who want to work in the PAF Air Defence Branch, Navy Weapon Engineering Branch, or Ordnance Branch of the Navy can find considerable advantages in practicing these multiple-choice questions. Furthermore, because the chemical bonding multiple-choice questions (MCQs) cover a wide range of mathematics topics, students who want to do well on the Army Navy and Pakistan Air Force entrance exams will find them invaluable.

Chemical Bonding (Part-5)

  • The intermolecular force responsible for capillary action in a narrow tube is the ________ force. (glue)
  •  The intermolecular forces that exist between an ion and a polar molecule are called ________ forces. (ion side)
  • The intermolecular forces between two separate ions are called ________ forces. (ion-ion)
  • The intermolecular force between the positive end of one molecule and the negative end of another molecule are called ________ forces. (dipole-induced dipole)
  • The intermolecular forces between a polar molecule and a nonpolar molecule are called ________ forces. (Dipole-Induced Dipole)
  • Bond energy is the ________ required to break a bond. (Energy)
  • The bond length is ________ between the nuclei of two bonded atoms. (Distance)
  • The shorter the bond length, the ________ bond. (Stronger)
  • Bond energy is usually expressed in units of ________. (kilojoules per mole)
  • Bond length is usually expressed in units of ________. (Picometers)
  • In general, triple bonds have ________ bond energy and ________ bond length compared to double bonds. (Higher, Lower)
  • In a molecule with multiple bonds, the bond with the ________ bond order is usually the one with the highest bond energy. (Highest)
  • Bond energy is determined by the ________ between the bonded atoms. (Attraction)
  • Bond length is affected by the ________ between the bonded atoms. (Size of atoms)
  • The bond energy of a covalent bond is proportional to the ________ of the atoms involved in the bond. (Electronegativity)
  • The bond length of a covalent bond is affected by the ________ number of atoms involved in the bond. (Atomic Radius)
  • The bond energy of a hydrogen bond (H-H) is ________. (436 kJ/mol)
  • The bond length of a carbon-carbon (C-C) single bond is ________. (about 154)
  • The bond energy of a carbon-oxygen (C=O) double bond is ________. (about 745 kJ/mol)
  • The bond length of a nitrogen-nitrogen (N-N) triple bond is ________. (around 110 pm).

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