Question

how do i write the symbols and information?

• hyphen notation
• element name followed by the mass number
• ________________________________
• used to differentiate between two isotopes of the same element
• example:

carbon – 14 uranium-238
p p
n⁰ n⁰
e⁻ e⁻

• standard nuclear notation
• also used to represent an isotope

1.
2.

1. 4.

isotopes

• atoms of the same element having the _______________, but _________________.
• isotopes of the same element have different atomic masses and mass numbers.
• isotopes of the same element are chemically alike because they have the

__________________________.
difference between ions and isotopes
ions and isotopes are __________________.

1. ions involve ____________________.

a. note: __________________ remains the same and does not change, otherwise the
element would change !!!!!!

1. isotopes involve ____________________.

average atomic mass

• the ___________________ in it on the periodic table
• the average atomic masses of an element is calculated from ___________ of the element

________________________

• a relative standard value for the mass of atoms defined by the carbon - 12 atom
• 1 amu = _____________________ = 1.66 x 10⁻²⁴ g
• the ___________________ in existence
• the ___________________ of each isotope
• the ______________ of each isotope

Explanation:

Fills in the blanks based on core chemistry concepts for isotopes, nuclear notation, ions, and average atomic mass.

Answer:

Hyphen notation

• Element name followed by the mass number
• Same atomic number (proton count)
• Used to differentiate between two isotopes of the same element
• Example: Carbon-14, Uranium-238

Isotopes

• Atoms of the same element having the same number of protons (atomic number), but different number of neutrons (neutron count).
• Isotopes of the same element are chemically alike because they have the same number of valence electrons.

Difference between Ions and Isotopes

Ions and isotopes are different types of atomic variations.

1. Ions involve a change in the number of electrons (gain/loss).

a. Note: Number of protons (atomic number) remains the same and does not change, otherwise the element would change !!!!!!

1. Isotopes involve a change in the number of neutrons.

Average Atomic Mass

• The atomic mass value listed in it on the periodic table
• The average atomic masses of an element is calculated from the isotopic composition of the element
• A relative standard value for the mass of atoms defined by the carbon-12 atom
• 1 AMU = $\frac{1}{12}$ the mass of a carbon-12 atom = $1.66 \times 10^{-24}$g
• The naturally occurring isotopes in existence
• The relative natural abundance of each isotope
• The mass number (isotopic mass) of each isotope