Atomic Structure and isotopes Flashcards
What charge do atoms have?
Neutral
what is the structure of an atom?
-Most= empty space between the nucleus and the electron shells
What are the properties of the nucleus?
Compared with a total, volume of the atom, nucleus is tiny and extremely dense
What are electrons held in place by?
an Electrostatic attraction from the nucleus
what are nucleides?
A term used to describe any atom of which the atomic number and the mass number are specified
What is the mass (nucleon number) defined as?
The number of protons and neutrons are present in the nucleus of the atom
what is the atomic number (proton number) defined as?
The number of protons present in the nucleus of the atom
how do you find the number of electrons in a negative ion (anion)?
add the charge to the atomic number
how do you find the number of electrons in a positive ion (cation)?.
Subtract the charge from the atomic number?
what does isoelectronic mean?
Atoms and ions that have the same number of electrons
What are isotopes?
Atoms of the same element with different numbers of neutrons and different masses
why do isotopes have similar chemical properties?
Because they have the same electronic structure
why my isotopes have slightly varying physical properties?
Because they have different masses
what is relative atomic mass?
The weighted mass of all the isotopes- taking into account the relative abundance of isotopes
What is the relative atomic mass equation?
isotopic mass x % abundance/ 100
isotopic mass x Relative abundance/ total relative abundance.
when do use the second relative atomic mass equation?
if the relative abundance is used instead of percentage abundance
what is relative atomic mass of an element?
The weighted mean mass of an atom of an element, compared with 1/12th mass of an atom of carbon 12, which has a mass of 12
What is the relative isotopic mass for an isotope?
The mass of an isotope of, compared with 1/12th mass of an atom of carbon 12, which has a mass of 12
what is relative molecular mass?
avg mass of molecule, compared with 1/12th mass of an atom of carbon 12, which has a mass of 12
