chemisty Multiple choice

Q3

1) Which of the following represents a measured value?

A) 36 inches = 1 yard

B) 77.0 miles from Russellville to Little Rock

C) 1000 microliters = 1 milliliter

D) two of the above

2) Which of the following is not a fundamental unit of the metric system?

A) meter B) liter C) pound

C) gram

3) Which of the following represent a ‘compound’ unit”

A) g/ml B) milliliter C) kilogram

D) meter

4) What is its density, in g/cm3, if 50.0 g of osmium has a volume of 2.22 cm3?

A) 0.0444 g/cm3 B) 22.5225 g/cm3 C) 4.4 x10-2 g/cm3

D) 22.5 g/cm3

5) If the density of milk is 1.04 g/mL, how many grams of milk are in 0.50 qt?

(1 qt = 0.946 L, 1L = 1000mL)

A) 1.04g B) 490g C) 13.2 g

D) 491.82 g

Q7

1) The atomic number represents _______.

A) The number of electrons in the element.

B) The number of protons in the element.

C) The number of neutrons in the element.

D) The mass number.

2) Elements having identical symbols but differing mass numbers are known as ____.

A) cations B) anions

C) isotopes D) isomorphs

3) The difference between atomic number and mass number for an element is related to the number of _____ in an atom.

A) electrons B) protons

C) quarks D) neutrons

4) Why is the mass number not a whole number?

A) It represents the average number of neutrons in all of the isotopes.

B) Electrons don’t weigh in whole numbers.

C) Protons don’t weigh in whole numbers.

D) Neutrons don’t weigh in whole numbers.

5) Isotopes are always radioactive.

A) True B) False

C) D)

Q8

1) Chemistry involving changes in the nucleus of an atom is referred to as _____ chemistry.

A) core B) nuclear

C) interior D) anthropomorphic

2) Isotopes are defined as those atoms of an element that have different ____ in the nuclei.

A) number of protons B) number of electrons

C) number of anti-protons D) number of neutrons

3) In isotope symbols, the mass number and atomic number are _____.

A) in identical positions B) on the opposite side (right vs left)

C) in opposite positions (top vs bottom) D) the same number

4) All isotopes are infinitely stable.

A) True B) False

C) D)

5) All isotopes are man-made.

A) True B) False

C) D)

Q9

1) Radioactivity is defined as _____.

A) disintegration of an unstable nucleus

B) absorption of particles into the nucleus

C) absorption of radio frequency energy

D) none of these

2) Half-life is defined as _____.

A) half a sample is gone

B) a sample glows at half intensity

C) the time required for ½ of a sample to emit

D) all of these

3) A half-life plot is a ___ graph.

A) linear B) exponential

C) inverse D) can’t be plotted

4) All radioactive decays produce a stable end product.

A) True B) False

C) D)

5) All radioactive isotopes are naturally occurring.

A) True B) False

C) D)

Q11

1) Regarding to energy levels, what happens to an arbitrary atom’s electrons when it absorbs a photon?

A) The electrons rise in energy levels B) The electrons lower in energy levels  

C) nothing happens to the electrons D) the phases of the moon change

2) What is the maximum number of electrons in an energy level (n) equal to?

A) 2n3 B) n

C) 2n2 D) 3n3

3) What is the shape of a s-orbital of an arbitrary atom.

A) sphere B) four-leaf clover

C) dumb-bell D) sunflower

4) What is the electron configuration of He?

A) 1s22s2

B) 1s0

C) 1s1

D) 1s2

5) How many types of sublevels are there?

A) 2 B) 3

C) 4 D) 10

Q13

1) What two types of elements compose an ionic compound?

A) metal-nonmetal B) nonmetal-nonmetal

C) metal-metal D) all of the above

2) In an ionic bond, the anion (negative ion) --- the electron from the cation (positive ion).

A) steals B) shares

C) both D) neither

3) Which is an ionic compound?

A) sugar B) aluminum

C) salt D) oxygen gas

4) What is the chemical formula for sodium sulfide?

A) NaS

B) Na2S

C) NaS2

D) Na2S2

5) From the chemical formula in question four, what was the cation (charge) and the anion (charge)?

A) Na (+1); S (-1) B) Na (+2); S (-1)

C) S (+1); Na (-1) D) Na (+1); S (-2)

Q15

1) What is the octet rule?

A) The want for an atom in a compound to retain eight electrons in its most outer shell of electrons

B) The want for an atom in a compound to retain two electrons in its most outer shell of electrons

C) A and B

D) none of the above

2) What doesn’t an electron-dot formula show?

A) The sequence of bonded atoms in a molecule or polyatomic ion

B) The central atom bonded to other atoms

C) The nonbonding pairs of protons shared between atoms

D) The nonbonding or unshared (lone pairs) of electrons

3) What is the electron-dot formula for water?

A) H:O:H B) H:O:H

C) O::H:H D) H:::O:H

4) What is the electron-dot formula for ammonia?

A) H N H

H

B) H N H

H

C) H N H

H

D) H N H

H

5) How many total electrons are in phosphorous trichloride (PCl3)?

A) 22 B) 26

C) 25 D) 27

Q17

1) What is the bond angle for a molecule with a tetrahedral geometry?

A) 120 B) 180

C) 109 D) 360

2) Which molecule has a tetrahedral molecular geometry?

A) methane B) water

C) ammonia D) carbon dioxide

3) What is the molecular geometry for ammonia?

A) linear B) trigonal pyramidal

C) bent D) tetrahedral

4) Which compound is an example of an alcohol?

A) CH4 (methane)

B) CH3CH2OH (ethanol)

C) CH3COOH (acetic acid)

D) C6H6 (benzene)

5) Which two functional groups are in every amino acid?

A) amines and carboxylic acids B) alcohols and ethers

C) alcohols and amines D) ethers and esters