1.1 Atoms, Electrons, And Orbitals

Question 1

Schroedinger calculated energy in hydrogen atom by using equations that treated the electron _

Answer 1

As if it were a wave

Question 2

Instead of a single energy, schroedinger obtained _

Answer 2

Series of energies

Question 3

Each of the series of energies corresponded to a different _

Answer 3

Mathematical description of the electron wave

Question 4

The mathematical descriptions are called _

Answer 4

Wave functions

Question 5

Wave functions symbolized by Greek letter

Answer 5

Psi 🔱

Question 6

Probability of finding an electron at a particular spot from nucleus

Answer 6

Square wave function

Question 7

Most stable state of hydrogen atom is _

Answer 7

Lowest energy

Question 8

Probability of finding electron at particular point is greatest towards _

Answer 8

Nucleus

Question 9

Probability of finding an electron decreases as you distance from nucleus but never

Answer 9

Becomes zero

Question 10

Wave functions are also called _

Answer 10

Orbitals

Question 11

_ can be used in several different ways

Answer 11

Term orbital

Question 12

Orbitals described by their size, shape and _

Answer 12

Directional properties

Question 13

Spherically symmetrical orbitals are called _

Answer 13

S orbitals

Question 14

Letter s preceded by _ n

Answer 14

Principal quantum number

Question 15

N specifies shell and is related to _

Answer 15

Energy of the orbital (n = 1, 2, 3, etc.)

Question 16

An electron on a 1s orbital is likely to be found _ and is lower energy

Answer 16

Closer to nucleus

Question 17

Electron 1s more strongly held than _

Answer 17

2s

Question 18

Instead of probability distributions, more common to represent orbitals by _

Answer 18

Their boundary surfaces

Question 19

The region enclosed by a boundary surface is _

Answer 19

Arbitrary

Question 20

Arbitrary but is customarily the volume where

Answer 20

Probability of finding an electron is high (90-95%)