Ch2

Question 1

Nucleus contains

Answer 1

Proton, neutron

Question 2

Where are electrons located

Answer 2

It surrounds these nuclear and rotates around it at high speeds

Question 3

Why is the atom electrically neutral

Answer 3

Atoms are neutral because they have equal numbers of electrons and protons,
and hence the overall charge is zero.

Question 4

If electrons are lost from or added to a neutral atom, the atom will be charged and
is called an__, which may be a cation or anion.

Answer 4

ion

Question 5

Cation and anion charges and when are they formed

Answer 5

Cations (positive ions) are formed when a neutral atom loses one or more
electrons. So, the number of electrons is lower than the number of protons.

o Anions (negative ions) are formed when a neutral atom gains one or more
electrons. So, the number of electrons is higher than the number of protons.

Question 6

A specific atom is described by two numbers;

Answer 6

atomic number and mass
number

Question 7

Atomic number, Z:

Answer 7

is the number of protons in the atom’s nucleus

Question 8

What’s the atoms charge if the number of protons inside the nucleus is the same number
of electrons around the nucleus.

Answer 8

Neutral atom

Question 9

The mass number, A:

Answer 9

It is equal to the sum of neutrons and protons inside the atom’s nucleus.

Question 10

The identity of an element is controlled by its___ (the number of protons in the nucleus).

Answer 10

atomic number

Question 11

atoms of a given element have the same atomic number BUT Diffrent mass number due to diffrent numbers of neutron is called an

Answer 11

Isotope

Question 12

Electrons are arranged in energy levels, also called.

Answer 12

shells

Question 13

She’ll numb? Is the closest to the nucleus and has the lowest energy

Answer 13

1

Question 14

As the order of the shell is increased, its energy is___ and electrons are less tightly bound to
the nucleus.

Answer 14

increased

Question 15

T or f. Atoms can exist in specific energy states, and in each energy state, the atom
has a definite energy.

Answer 15

True

Question 16

When an atom has its electrons in their lowest possible energy levels, the
atom is in its__ (Lowest energy state).

Answer 16

ground state

Question 17

When the atom absorbs energy, one or more electrons will jump to a
higher energy level (promotion of electrons) and the atom changes its
energy state to the__ (highest energy state).

Answer 17

excited state

Question 18

Energy levels or shells contain

Answer 18

energy sublevels or subshells.

Question 19

The number of subshells per a certain energy level is_____. This is applicable until the fourth energy level.

Answer 19

equal to the order of the energy level

Question 20

How many subshells this energy level #4 has

Answer 20

four subshells

Question 21

True or false. Energy increase S<p<d<f

Answer 21

True

Question 22

Each energy sublevel contains.

Answer 22

orbitals

Question 23

is the volume of space around a nucleus where an electron spends most
of its time.

Answer 23

An orbital

Question 24

Completely filled orbital is the orbital that contains___.
o Half-filled orbital (singly occupied orbital) is the orbital that
contains one electron
o Vacant Orbital is the orbital that contains no electrons

Answer 24

two electrons.

Question 25

The s orbital is spherical, with the nucleus at its.

Answer 25

center

Question 26

What is the difference between the 1s orbital and the 2s orbital?.

Answer 26

1s lower energy and smaller and 2s higher energy and larger

Question 27

three___ are dumbbell–shaped and mutually perpendicular to each other, denoted px, py, and, pz

Answer 27

p orbitals

Question 28

How many orbitals and what’s the max numb of elect of S sub shell

Answer 28

Orbitals1 elec2

Question 29

play important roles in describing the energy levels of electrons and the shapes of the orbitals that describe the distributions of electrons in space.

Answer 29

quantum numbers

Question 30

The quantum numbers

Answer 30

Principal Quantum Number (n) ➢ Secondary (Subsidiary or Azimuthal) Quantum Number (ℓ) ➢ Magnetic Quantum Number (mℓ) ➢ Spin Quantum Number (ms)

Question 31

When two electrons occupy the same atomic orbital, they will have the same values of______ but different ms values because of their opposite spins.

Answer 31

n, ℓ, and mℓ

Question 32

Which principle is this, No two electrons in an atom may have identical sets of four quantum numbers

Answer 32

Pauli exclusion principle

Question 33

For L=3 how many orbitals can be found

Answer 33

2x3+1=7

Question 34

For n=2 how many orbitals can be found

Answer 34

n^2 =4

Question 35

How many electrons can the p orbital hold?

Answer 35

6

Question 36

__refers to the distribution of electrons of an atom in its orbitals

Answer 36

Electronic configuration

Question 37

Rules for filling electrons

Answer 37

Aufbau exclusion principle

Question 38

Which principle, Electrons of an atom occupy orbitals in the order of increasing orbital energy.”

Answer 38

Aufbau exclusion principle

Question 39

Which principle is this example from, Electrons fill the lowest energy orbitals first and then proceed to the higher energy one.

Answer 39

Aufbau exclusion principle

Question 40

The order of filling of atomic orbitals

Answer 40

1s 2s 2p 3s 3p 4s 3d……

Question 41

Which principle is this, “No two electrons in an atom may have identical sets of four quantum numbers.”

Answer 41

Pauli Exclusion Principle:

Question 42

Which principle is this from, 1s orbital can hold a maximum of two electrons and, when filled, the electrons must have opposite spins

Answer 42

(Pauli Exclusion Principle).

Question 43

Which rule is this , “Electrons must occupy all the orbitals of a given sublevel singly before pairing begins. These unpaired electrons have parallel spins.

Answer 43

Hund’s Rule

Question 44

Methods of writing electronic configurations

Answer 44

Orbital diagram, spdf notation, noble gas notation

Question 45

The electronic configuration for the orbital diagram is written according to the

Answer 45

Aufbau principle with respect to the Pauli Exclusion and Hund principles.

Question 46

Which is the most stable electron configuration and their subshells are completely filled

Answer 46

Noble gas notation