ATOMIC STRUCTURE AND BONDING IN SOLIDS part 1

Question 1

What is atomic structure?

Answer 1

Atomic structure refers to the structure of an atom.

Question 2

What is an atom’s structure?

Answer 2

An atom is made up of a center of positive charges called protons and none charges called neutrons, called the nucleus. negative charged called electrons revolve around the nucleus.

Question 3

what group of particles do protons and neutrons fall under?

Answer 3

nucleon

Question 4

electrons and protons have opposing charges of the same magnitude. true or false?

Answer 4

true!

Question 5

what is the charge of an electron?

Answer 5

1.60x10^-19 coulombs

Question 6

protons and neutrons have roughly equivalent masses of ~1.67x10^-27 but which is heavier?

Answer 6

neutrons

Question 7

what is atomic number?

Answer 7

the number of protons in a nucleus

Question 8

when is an atom neutral ?

Answer 8

when the number of proton is equal to the number of electrons

Question 9

atoms of the same element can have the same number of protons but different neutron number. true or false

Answer 9

true

Question 10

He^4
2
how many protons, neutrons and electrons are there in this element?

Answer 10

2 protons
2 neutrons
2 electrons

Question 11

how did you find the protons?
how did u find the electrons?
how did u find the neutrons?

Answer 11

the protons are the same as the atomic number the bottom number.
the number of electrons is the same as the number of protons.
the number of neutrons is equal to the mass number(the number at the top) - the proton (atomic) number.

Question 12

what are isotopes?

Answer 12

are the same element that have different atomic mass numbers due to different number of neutrons.

Question 13

what are the two atomic model

Answer 13

Bohr atomic model and
Wave-mechanical model

Question 14

what is a bohr atomic model

Answer 14

Bohr atomic models are scientist early attempt to describe the position and energy level of electrons in an atom. But it does not help example several phenomena involving electrons as it is to simplistic.

Question 15

Describe the characteristics of a Bohr atomic model

Answer 15

-Electrons revolve around an atomic nucleus in discrete orbitals.
- the position of any electron is defined in terms of its orbital
- Electrons have quantized/ specific energy levels
- electrons absorb energy in terms of photons when it makes a quantum jump to a higher energy level and emits energy when jumping to a lower energy level
-the energy of a photon is planks constant (h) * frequency of the proton.

Question 16

describe wave mechanical model

Answer 16

in a wave mechanical model electrons exabit both wave-like and particle-like characteristic.
the position of any electrons is calculated by the probability of it being at various location around the nucleus this is call probability distribution or an electron cloud

Question 17

Principle quantum number (n)

Answer 17

refers to the distance from the nucleus. n 1 being the closest

Question 18

secondary quantum number (l)

Answer 18

relates to the shape of the subshell. has letters s,p,d,f and it is limited by the value of n

Question 19

third quantum number (ml)

Answer 19

specifies the number of energy states for each subshell. s = 2, p= 6, d= 10, f= 14 and can go to infinity.

Question 20

fourth quantum number(ml)

Answer 20

specifies the spatial orientation for each electron’s spin moment (up or down) +1/2 or -1/2

Question 21

Pauli exclusion principle

Answer 21

This states that in an atom or molecule no two electrons can have the same four electronic quantum numbers( they can not take up the same position).
and each electron in the same orbital must have opposing spins.
this principle is used to determine the manner in which electrons are filled into shells

Question 22

what is ground state?

Answer 22

an atom is in its ground state when all electrons occupy the lowest possible energy levels

Question 23

what are valence electrons

Answer 23

these are electrons that occupy the outer most shell.
these outer most electrons participate in interatomic bonding and affect the physical and chemical properties of solids

Question 24

when does an atom achieve stability and how does it achieve this

Answer 24

when the atom has completely filled valence electron shells. it ca achieve this by losing or gaining electrons to form charged ions or by sharing electrons with other atoms

Question 25

state the electron configurations of - k - fe -fe3+

Answer 25

k = 19 1s2 2s2 2p6 3s2 3p6 4s1 fe = 26 1s2 2s2 2p6 3s2 3p6 4s2 3d6 fe3+ 1s2 2s2 2p6 3s2 3p6 3d5

Question 26

F, CL ,BR,I , AT are a group of elements known as

Answer 26

Halogens

Question 27

group 1 metals are known as

Answer 27

alkali metals

Question 28

group 2 metals are known as

Answer 28

alkali earth metals

Question 29

what is a transition element?

Answer 29

this is a d block element that forms one or more stable ions with complete d subshells

Question 30

what is an electro positive element

Answer 30

not all elements that lose electrons are metals thus we give the term for all elements that gain stability by the lose of electrons to form positively charged ions a electro positive

Question 31

what is an electro negative element

Answer 31

these are elements that have to gain electrons in order to gain stability by forming negatively charged ions Or by sharing electrons with other atoms as electro negative

Question 32

electronegativity increases across a group and up a period true or false?

Answer 32

true

Question 33

what factors do valence electrons determine in atomic bonding?

Answer 33

-chemical -optical -electrical -thermal

Question 34

what is bond energy in terms of attractive forces and repulsive forces formula?

Answer 34

En (net energy) = EA(attractive) + ER(replusive)