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Gen. chem exam 1

front 1

A pure substance composed of 2 or more different elements is a_____.

back 1

Chemical compound

front 2

Who is credited with measuring the mass charge ratio of an element?

back 2

J.J. Thompson

front 3

The Chemist credited for inventing a set of symbols for writing the formulas of a compound, and for discovering selenium, silicon, and thorium is _______.

back 3

Jöns Jacob Berzelius

front 4

The law of multiple proportions states that________________.

back 4

if multiple compounds can form from the same 2 elements, and the mass of one element is fixed, then the masses of the other element occur in small whole number ratios.

front 5

Mass fraction=

back 5

(Total mass of element in compound)/(Total mass of compound)

front 6

Which of the following postulates of Dalton's atomic theory are still scientifically accepted?

I.

All atoms of the same element are identical.

II.

Compounds are combinations of different atoms.

III.

A chemical reaction changes the way atoms are grouped together.

IV.

Atoms are indestructible.

back 6

II and III

front 7

T/F: The emission spectrum of hydrogen contains a continuum of colors.

back 7

False

front 8

Excited hydrogen atoms radiate energy in the___________.

back 8

infrared, visible and ultraviolet regions.

front 9

Which of the following statements are false?

I.

It takes less energy to add an electron to nitrogen than to carbon because nitrogen

will be closer to achieving a noble gas configuration.

II.

It takes more energy to add an electron to fluorine than to oxygen because the radius

of fluorine is smaller and more repulsion would occur in the p-orbitals.

III.

It takes more energy to add an electron to nitrogen than to carbon because of the

extra repulsions that would occur in the 2p orbitals.

IV.

Less energy is released in adding an electron to iodine than to chlorine because

the radius of iodine is larger and the electron is added at a distance further

from the nucleus.

back 9

I, II

front 10

What type of spectrum, if any, would be produced if the light radiated by a heated atomic gas were to be dispersed through a prism?

back 10

Discrete lines of different colors

front 11

T/F: A 2p orbital is more penetrating than a 2s; i.e., it has a higher electron density near the nucleus and inside the charge cloud of a 1s

back 11

False

front 12

The 2s orbital in calcium is more stable (more negative energy) than the 2p orbital even though the 2p orbital has its maximum electron density closer to the nucleus. The reason for this higher stability is:

back 12

due to its greater penetration, the 2s orbital has more electron density close to the nucleus than the 2p orbital

front 13

According to the Aufbau principle which sublevel is filled after the 5s sublevel?

back 13

4d

front 14

The Aufbau principle states that___________________.

back 14

electrons orbiting one or more atoms fill the lowest available energy levels before filling higher levels.

front 15

How many unpaired electrons are there in a manganese atom?

back 15

5

front 16

Ionization energy is_____________.

back 16

the energy required to remove an electron from a neutral atom.

front 17

Electron affinity is____________.

back 17

the energy change when a neutral atom attracts an electron to become a negative ion

front 18

Electronegativity is_______________.

back 18

the ability of an atom in a molecule to draw bonding electrons to itself.

front 19

T/F: Subshell energies are higher in multielectron atoms than the same subshell in the hydrogen atom.

back 19

False

front 20

T/F: In the hydrogen atom, all subshells of a principal shell are at the same energy level.

back 20

True

front 21

T/F: In a multielectron atom, the various subshells of a principal shell are at different energy levels.

back 21

True

front 22

T/F: All orbitals within a subshell of a multielectron atom are at the same energy level.

back 22

True

front 23

T/F: In high numbered principal shells of a multielectron atom, some subshells of different principal shells have nearly identical energies.

back 23

True

front 24

What is the maximum number of electrons that can occupy the n = 5 shell?

back 24

50

front 25

How many orbitals are there of the 4f type?

back 25

7

front 26

Areas of zero probability of finding an electron are called _________.

back 26

nodes or nodal surfaces

front 27

The statement that "the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals" is known as___________.

back 27

Hund's rule

front 28

Which of the following atoms or ions has three unpaired electrons?

back 28

N

front 29

Which of these pairs is incorrect?

back 29

gallium - main group nonmetal

front 30

Which one of the following equations correctly represents the process involved in the electron affinity of X?

back 30

X(g) + e¯ → X¯(g)

front 31

Which of the following statements is true?

back 31

The ionic radius of Fe+ is larger than that of Fe3+.

front 32

Which of the following compounds has the greatest bond polarity?

back 32

HF

front 33

Consider the following elements: Si, Co, Cl, P, Sr, F, Rb
Select the most accurate statement.

back 33

Co, Sr, and Rb will form ionic compounds with Cl and F

front 34

In the reaction between magnesium and sulfur, the magnesium atoms

back 34

become cations

front 35

Give the name and formula of the compound whose molecules consist of two iodine atoms and seven oxygen atoms.

back 35

diiodine heptaoxide; I2O7

front 36

Using the following bond energies:

Bond Bond Energy (kJ/mol) C≡C 839 C–H 413 O=O 495 C=O 799 O–H 467 estimate the heat of combustion (ΔE) for one mole of acetylene: C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(g)

back 36

–1228 kJ

front 37

In the cyanide ion (CN–), the nitrogen has a formal charge of

back 37

0