Chemistry

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Showing 1001 to 1025 of 1398 questions (page 41 of 56).

1001. Dalton's law of partial pressures does not apply to gases that

A. are at high temperature B. are monatomic C. have different molar masses D. react chemically with each other E. are at low pressure

1002. The abnormally high boiling point of water compared with hydrogen sulphide is due to

A. London dispersion forces B. hydrogen bonding C. its ionic character D. covalent network bonding E. its low molar mass

1003. The boiling point of a liquid at reduced external pressure

A. decreases B. becomes zero C. doubles D. increases E. remains unchanged

1004. The coordination number of each ion in a sodium chloride crystal is

A. 12 B. 8 C. 2 D. 4 E. 6

1005. The existence of a substance in more than one crystalline form is called

A. allotropy in solutions only B. anisotropy C. polymorphism D. isomorphism E. isotopy

1006. Which type of solid has the highest melting point?

A. amorphous B. metallic C. covalent network D. ionic E. molecular

1007. The maximum number of electrons that can occupy the shell with n = 3 is

A. 10 B. 6 C. 8 D. 32 E. 18

1008. For an electron in a 3d orbital, the azimuthal quantum number l is

A. 2 B. 3 C. 1 E. 4

1009. The ground state electronic configuration of chromium (Z = 24) is

A. [Ar] 4s2 4p4 B. [Ar] 3d5 4s1 C. [Ar] 3d6 D. [Ar] 3d3 4s3 E. [Ar] 3d4 4s2

1010. Rutherford's gold foil experiment established the existence of

A. a small dense positively charged nucleus B. the neutron C. orbitals D. the electron E. energy levels

1011. The energy of a photon of frequency nu is given by

A. h/nu B. h nu C. h nu2 D. nu/h E. h/nu2

1012. The shape of a p orbital is

A. spherical B. tetrahedral C. planar triangular D. double dumb bell E. dumb bell

1013. Hund's rule requires that

A. d orbitals fill before s orbitals of the same shell B. the lowest energy orbital is filled last C. degenerate orbitals are singly occupied with parallel spins before pairing D. electrons pair up before occupying empty degenerate orbitals E. no two electrons can have the same spin

1014. The bond angle in a molecule with sp3 hybridization and no lone pairs is

A. 107 degrees B. 120 degrees C. 109.5 degrees D. 104.5 degrees E. 90 degrees

1015. The dipole moment of carbon dioxide is zero because the molecule is

A. tetrahedral B. linear and symmetrical C. non-polar in its bonds D. ionic E. angular

1016. The shape of the ammonia molecule according to VSEPR theory is

A. trigonal pyramidal B. trigonal planar C. tetrahedral D. linear E. bent with 104.5 degrees

1017. As bond order increases, the bond length

A. remains constant B. first increases then decreases C. increases D. decreases E. becomes zero

1018. A coordinate covalent bond is present in

A. ethene B. methane C. sodium chloride D. chlorine E. the ammonium ion

1019. The ionic character of a bond increases with

A. increasing covalent radius B. decreasing atomic size only C. increasing electronegativity difference D. decreasing electronegativity difference E. increasing bond order

1020. In benzene, all six carbon to carbon bonds are of equal length because of

A. sp3 hybridization B. ionic character C. free rotation D. hydrogen bonding E. resonance delocalization

1021. The hybridization of carbon in ethyne is

A. sp2 B. sp C. sp3 D. sp3d E. unhybridized

1022. For an exothermic reaction, the enthalpy change is

A. negative B. zero C. always equal to the activation energy D. positive E. undefined

1023. Hess's law states that the enthalpy change of a reaction

A. depends on the path taken B. depends only on temperature C. equals the activation energy D. is independent of the path taken E. is always negative

1024. The standard enthalpy of formation of an element in its most stable form is

A. equal to its bond energy B. always negative C. always positive D. equal to its atomization energy E. zero

1025. The enthalpy of neutralization of a strong acid by a strong base is nearly constant because

A. the reaction is always the combination of H+ and OH- to give water B. the reaction is endothermic C. all acids have the same concentration D. the salts formed are identical E. water is a catalyst

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