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Friday, June 17, 2016

Exercise Chemistry

1. The ion that isoelectronic with CO is
2. Which of the following contains a covalent bond?
3. How are bond length and bond energies related?
 the lower the bond energy, the shorter the bond length
 the higher the bond energy, the longer the bond length
 they are not related
 the higher the bond energy, the shorter the bond length
4. A strontium atom differs from a strontium ion in that the atom has a greater
 mass number
 atomic number
 number of electrons
 number of protons
5. which one among the following does not have the hydrogen bond?
 liquid HCl
 liquid NH3
6. Which bond has the greatest ionic character?
7. Which type of bonding would be expected between S and Cl?
 non-polar covalent
 polar covalent
8. On hybridization of one s and one p orbitals we get:
 four orbitals directed tetrahedrally
 three orbital in a plane
 two orbital at 180°
 two mutually perpendicular orbitals
9. The bond between two identical non-metal atoms has a pair of electrons:
 unequally shared between the two
 transferred fully from one atom to another
 with identical spins
 equally shared between them
10. the molecule having one unpaired electron is:
11. Which formula represents a molecular substance?
12. Which kinds of bonding can be found in a sample of H2O(l)?
 Hydrogen bonds only
 Nonpolar covalent bonds only
 Ionic and nonpolar hydrogen bonds
 Both polar covalent and hydrogen bonds
13. Which substance has a polar covalent bond between its atoms?
14. Which substance is an example of a network solid?
 silicon dioxide
 nitrogen dioxide
 sulfur dioxide
 carbon dioxide
15. Atoms bond primarily to _____.
 make more atoms
 reduce their potential energy and gain stability
 increase thier potential energy and lose stability
 increase their potential energy and gain stability
16. When an ionic compound is dissolved in water, the ions in solution can best be described as
 hydrated molecules only
 hydrated ions only
 dehydrated ions and molecules
 both hydrated molecules and hydrated ions
17. Polar refers to _____.
 even-sized electronegativities in a bond
 the formation of uneven size ions
 bonds that have an even distribution of charge
 bonds that have an uneven distribution of charge
18. carbon tetrachloride has no net dipole moment because of
 its regular tetrahedral structure
 similar electron affinities of carbon and chlorine
 its planar structure
 similar sizes of carbon and chlorine atoms
19. Which combination of atoms can form a polar covalent bond?
 H and Br
 Na and Br
 H and H
 N and N
20. Which sequence of Group 18 elements demonstrates a gradual decrease in the strength of the Van der Waals forces? All the choices are elements in the liquid state.
 Kr, Xe, Ar, Ne
 Ne, Ar, Kr, Xe
 Ar, Kr, Ne, Xe
 Xe, Kr, Ar, Ne
21. The force of attraction between oppositely charged ions in a compound is called
 a magnetic force
 an ionic bond
 a covalent bond
22. Which one of the following properties does not belong to a covalent substance?
 High melting point and a brittle solid.
 Insoluble in water and does not conduct electricity.
 Liquid with a low boiling point
 Soft solid and a very poor conductor of electricity
23. Which one of the following radicals is written with the incorrect formula?
24. What is the reason for ionic compounds having high melting and boiling points?
 Ionic compounds consist of a giant crystalline structure
 A small amount of energy is needed to break the bonds between the ions
 The bonds between the ions are strong
 The bonds between the atoms are strong
25. What is meant by a covalent bond?
 The transfer of electrons between two atoms
 The sharing of protons between atoms
 The attraction between two oppositely charged ions
 The sharing of electrons between atoms