proton 6
neutron 7
what is the atomic number ?
_______________________________________
To find the atomic number, you look at the number of protons.
-
Protons = 6 → So, the atomic number is 6.
This element is Carbon (C) on the periodic table.
-
Neutrons = 7 → This means it is an isotope of carbon, specifically Carbon-13 (6 protons + 7 neutrons = mass number 13).
✅ Final Answer:
Atomic number = 6
Element = Carbon (C)
Isotope = Carbon-13
_____________________________________________________________________________________ 3 isotopes =
classics example of carbon 6^C
isotopes
variation don't change
various form of carbon isotopes
carbon 13 and carbon 14
each one of these carbon have 6 carbon atoms
atomic mass is one additional neutron in there
how many neutron found in that element
carbon atomic number 1s 14
carbon proton 6
carbon Neutron 14-6= 8
_______________________________________________
ION is atom or a group of atom
atom we have protons (positive charge )
surrounding we have electron ( negative charge)
Na+ sodium ( 11 proton are blue ) and (11 electron are yellow )
cannot lose electron
sodium lose one electron if lose 1 electron
atom lose electron
Na + (cat ion) carries positive charge
oxygen 8 proton 8 electron net charge is 0
gain and lose electron
proton
10 electron at outside
(2 extra electron compare to the proton ) ( two negative charges ) negative charged ion is called anion
shell 1st shell n==1 (k-shell )
2nd shell n=2 (L=L shell s,p)
n=3 M shell - s, p ,f
n=4
SPDF
number of electron
we can only have 2 electron on that sub shell
how to characteristic on s shell (1st-S shell )
(2nd shell ) second energy level ( can have 8 electron at most) 1s2,2s2, 2p6
The subshell configuration for carbon (C) is based on its atomic number, which is 6. This means it has 6 electrons.
๐งช Carbon Electron Configuration (Subshells):
1s² 2s² 2p²
Breakdown:
-
1s² → 2 electrons in the 1s subshell
-
2s² → 2 electrons in the 2s subshell
-
2p² → 2 electrons in the 2p subshell
Summary:
-
Carbon has electrons in the 1s, 2s, and 2p subshells.
-
Total electrons: 6
-
Subshells: 1s² 2s² 2p² ✅
(3rd shell ) third energy level ( S, P ,D ) D shell maximum of 10
chemical bond formed two or more atom interact primarily through the outermost shell or energy level
they do not have 8 electron in their outer most shell
octet rule -
2 main type of bond ionic bond and covalent bond
sodium has atomic number 11
Proton 11
electron 11
1 st shell 2
2nd shell 8
positively charge
creation of sodium ion
chlorine 17 proton and 18 electrons
chloride ion 17
leading to the formation of sodium chloride
covalent bond - 2 atom share one or more electron
carbon - oxygen- hydrogen-nitrogen
octect rule -
carbondixoide - 8 proton and 8 electron
2 more electrons to complete outermost shell
innershell
4 addition atom to maintain
What is the correct electron configuration for Oxygen (atomic number 8)?
A. 1s² 2s² 2p³
B. 1s² 2s² 2p⁴
C. 1s² 2s¹ 2p⁵
D. 1s² 2s² 2p⁵