Chapter 4: Modern Atomic Theory

key advances made by the quantum theory model of the atoms

basically discovery of orbitals

orbital

an electron cloud where the electron could be anywhere in that cloud

Orbit

a place where the electron def is like it's there no question about it and it cannot move around it can only go from one orbit to another

how many electrons can be in each atomic orbital

2

total electron capacity of s

2

total electron capacity of p

6

total electron capacity of d

10

total electron capacity of f

14

Aufbau Principle

in the ground state of an atom or ion, electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels (e.g., 1s before 2s). In this way, the electrons of an atom or ion form the most stable electron configuration possible

Pauli Exclusion Principle

An orbital can only hold 2 electrons which must have opposite charges

Hund's Rule

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

ionization energy

The amount of energy required to remove the most loosely bound electron, the valence electron.

periodic trends for atomic size

Increase

|

|

|

------------> v

decrease

periodic trends for ionization energy

decrease

|

|

|

------------> v

Increase

Octet Rule

Elements react to form compounds in such a way as to put 8 electrons in their outermost valence shell-shell configuration identical to that of a noble gas and making them exceptionally stable

Uncertainty Principle

In dealing with particles the size of an electron it is impossible to know with any real accuracy exactly where the electron is or where it's going

What gave schrodinger justification to think of an electron in an atom as a nebulous cloud

Heisenberg's uncertainty principle, by stating that it is impossible to exactly locate an electron.

If an electron couldn't be exactly located in a volume of space, Schrödinger reasoned,

it could be thought of as being everywhere in that volume at once, filling it like a cloud.

d.) frequency times wavelength.

For electromagnetic radiation, c (the speed of light) equals_________.

a.) frequency minus wavelength

b.) frequency plus wavelength.

c.) frequency divided by wavelength.

d.) frequency times wavelength.

b.) frequency

One of the wave properties of electromagnetic radiation, such as light, is ____________.

a.) volume

b.) frequency

c.) mass

d.) weight

c.) the energy of the light is too low.

According to the particle model of light (photoelectric effect), certain kinds of light cannot eject electrons from metals because __________.

a.) the mass of the light is too low

b.) the frequency of the light is too high

c.) the energy of the light is too low

d.) the wavelength of the light is too short.

b.) shorter

If electromagnetic radiation A has a higher frequency than electromagnetic radiation B, the compared to B the wavelength of A is ________.

a.) longer

b.) shorter

c.) equal

d.) exactly half the length of B's wavelength

b.) wavelength

The distance between two successiv peaks (crests) on a wave is its _____.

a.) frequency

b.) wavelength

c.) quatum number

d.) velocity

a.) photon

A quantum of electromagnetic energy is called a(n) ______.

a.) photon

b.) electron

b.) excited atom

d.) orbital

c.) frequency

The energy of a photon, or quantum, is related to its ____________.

a.) mass

b.) speed

c.) frequency

d.) size

b.) to a lower energy level

A line spectrum is produced when an electron moves from one energy level _________.

a.) to a higher energy level

b.) to a lower energy level

c.) into the nucleus

d.) to another position in the same sublevel

c.) 4-5 distinct lines of different colors

When the pink-colored light of glowing hydrogen gas passes through a prism, it is possible to see ________.

a.) all the colors of the rainbow

b.) only lavender-colored lines

c.) 4-5 distinct lines of different colors

d.) black light

c.) released photons of only certain energies

Because excited hydrogen atoms always produce the same line-emission spectrum, scientists concluded that hydrogen ________.

a.) had no electrons

b.) did not release photons

c.) released photons of only certain energies

d.) could only exist in the ground state

d.) line-emission spectrum

The Bhor model of the atom was an attempt to explain hydrogen's _____.

a.) density

b.) flammabliity

c.) mass

d.) line-emission spectrum

b.) energy must be absorbed

For an electron in an atom to change from the ground state to an excited state,

a.) energy must be released

b.) energy must be absorbed

c.) radiation must be emitted

d.) the electron must make a transition from a higher to a lower energy level

a.) ground state

If electrons in an atom have the lowest possible energies, the atom is in the ,

a.) ground state

b.) inert stae

c.) excited state

d.) radiation-emitting state

b.) only the spectrum of hydrogen

Bhor's model of the atom works best in explaining

a.) the spectra of the first ten elements

b.) only the spectrum of hydrogen

c.) only the spectra of atoms with elections in an s orbital

d.) the entire visible spectra of atoms

a.) in specific, allowed orbits, depending on its energy

According to the Bohr model of the atom, the single electron of a hydrogen atom circles the nucleus

a.) in specific, allowed orbits, depending on its energy

b.) in one fixed orbit at all times

c.) at any of an infinite number of distances, depending on its energy

d.) counterclockwise

d.) the Bohr model of the atom explains the reactivity of all atoms.

All of the following statements are correct EXCEPT

a.) according to the Bohr model of the atom, the single electron of a hydrogen atom circles the nucleus in specific, allowed orbits

b.) the quantum model uses probability to locate the electon within the atom

c.) the orbitals of the quantum model of the atom were suggested by descriptions of electrons as waves

d.) the bohr model of the atom explaions the reactivity of all atoms

b.) the quantum model

Which model of the atom explains the orbitals of electrons as waves?

a.) the Bohr models

b.) the quantum model

c.) Rutherford's model

d.) Planck's theory

d.) it helps to locate a proton in an atom.

All of the following describe the Heisenberg uncertainly principle EXCEPT

a.) it states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle.

b.) it is one of the fundamental principles of our present understanding of light and matter

c.) it helped lay the foundation for the modern quantum theory.

d.) it helps to locate a proton in an atom

d.) it is the same as the Bohr's theory

All of the following describe the Schrodinger wave equation EXCEPT

a.) it is an equation that treats electrons in atoms as waves

b.) only waves of specific energies and frequencies provide solutions to the equation.

c.) it helped lay the foundation for the moder quantum theory.

d.) it is the same as the Bohr's theory

c.) orbital

A three-dimensional region around a nucleus where an electon may be found is called a(n)

a.) spectral line

b.) electron path

c.) orbital

d.) electron elipse

c.) magnetic quantum number

The quantum number that indicates the position of an orbital about the three axes in space is the

a.) principal quantum number

b.) angular momentum (orbital) quantum number

c.) magnetic quantum number

d.) spin quantum number

b.) atomic orbitals

Quantum numbers are sets of numbers that describe the properties of

a.) the atomic nucleus

b.) atomic orbitals

c.) atoms

d.) molecules

d.) principal quantum numbers

The main energy levels of an atom are indicated by the

a.) orbital quantum numbers

b.) magnetic quantum numbers

c.) spin quantum numbers

d.) principal quantum numbers

b.) ½ or -½

The possible values of an electron's spin quantum number are

a.) -1, 0, or 1

b.) ½ or -½

c.) 1 or -1

d.) 0 or 1

b.) p orbitals

The set of orbitals that are peanut-shaped and directed along the s, y, and z axes are called

a.) d orbitals

b.) p orbitals

c.) f orbitals

d.) s orbitals

a.) an s orbital

A spherical electron cloud surrounding an atomic nucleus would best represent

a.) an s orbital

b.) a px orbitral

c.) a combination of px and py orbitals

d.) a combination of an s and a px orbital

c.) the 2s orbital is at a higher energy level

The major difference between a 1s orbital and a 2s orbital is that

a.) the 2s orbital can hold more electrons

b.) the 2s orbital has a slightly different shape

c.) the 2s orbital is at a higher energy level

d.) the 1s orbital can have only one electron

d.) 3f

An orbital that could never exist according to the quantum description of the atom is

a.) 3d

b.) 8s

c.) 6d

d.) 3f

b.) the Aufbau principle

The statement that an electron occupies the lowest available energy orbital is

a.) Hund's rule

b.) Aufbau principle

c.) Bohrs' law

d.) the Pauli exclusion principle

d.) Hund's rule

"orbitals of equal eneregy are each occupies by one electron before any is occupies by a second electron, and all electrons in singly occupies orbitals must have the same spin" is a statement of

a.) the Pauli exclusion principle

b.) the Aufbau principle

c.) the quantum effect

d.) Hund's rule

a.) the Pauli exclusion principle

The statement that no two electrons in the same atom can have the same four quantum numbers is

a.) the Pauli exclusion principle

b.) Hund's rule

c.) Bohr's law

d.) the Aufbau principle

b.) occupies the lowest available energy level

The Aufbau prinicple states that an election

a.) can have only one spin number

b.) occupies the lowest available energy level

c.) must be paired with another electron

d.) must enter an s orbital

d.) 5s

The atomic sublevel with the next highest energy after 4p is

a.) 4d

b.) 4f

c.) 5p

d.) 5s

b.) octet

If the s and p orbitals of the highest main energy level of an atom are filled with electrons, the atom has a(n)

a.) electron pair

b.) octet

c.) ellipsoid

d.) circle