Chapter 2- Elements Of The Periodic Table Flashcards
What do atoms make up
all matter
What are atoms composed of
Protons, neutrons, electrons
What is mass of atom determined by
Mostly mass of nucleus
What is diameter of atom determined by
Cloud of electrons
Protons are
Positively charged
Neutrons are
Neutral
Electrons are
Negatively charged
Where are protons and neutrons found
In the nucleus
Where are electrons found
Outside of the nucleus
The charges of protons and electrons are
Equal but opposite
What does an element contain
Atoms of the same type
How can you find the number of protons/ electrons in an element
The atomic number
A-Z=
Number of neutrons
What are isotopes
Atoms with the same atomic number but different mass numbers
What are ions
Atoms that have lost or gained electrons to become charged particles
What is the emission spectra
When atoms are heated, they can emit electromagnetic radiation in the form of coloured light. When light is passed through a prism it produces a spectrum made up of lines of different colours
What is the Bohr model
The first atomic model to explain origin of emission spectra
What does the Bohr model assume
Electrons only exist in fixed, circular orbits if specific energies which later came to be known as energy levels or shells
What does each line in the emission spectrum correspond to
A specific electron transition between shells
How to calculate how many electrons each shell can hold
2n(squared)
How many electrons can the valance shell contain
No more than eight
What is oxidation
Additional of oxygen to a substance or removal of hydrogen from a substsnce
What is the octet rule
atoms will lose, gain or share electrons so that they can achieve 8 valence electrons as this is stable
What are the limitations of the Bohr model
1- no reason why a shell like the 3d would only fill up to 8.
2- cannot predict emission spectra of elements with more than one electron
3- is unable to explain why shells hold 2n(squared) electrons
What does the Schrodinger model suggest
electron shells are further divided into subshells
what are the subshells labelled as
s,p,d,f
What are orbitals
subshells are split into orbitals
how many electrons can an orbital hold
2 electrons
how many subshells does the first shell have (labelled)
1 (s)
how many subshells does the second shell have (labelled)
2 (s, p)
how many subshells does the third shell have (labelled)
3 (s, p, d)
what is the max electrons shell 1 can have
2
what is the max electrons shell 2 can have
8
what is the max electrons shell 3 can have
18
how many orbitals does the s subshell have
1
how many orbitals does the p subshell have
3
how many orbitals does the d subshell have
5
What is a ground state of an atom
has the electrons in the lowest possible energy subshells
What happens if an atom is in an excited state
when if energy is supplied to the atom, one or more of the outer electrons can jump into the next subshell
What are the exceptions for subshell configuration
Chromium and Copper
what do horizontal rows of the period table represent
periods labelled 1-7
what do vertical columns of the periodic table represent
groups, labelled 1-8
what do valence electrons give their elements
chemical properties
what are critical elements
elements that exist in small quantities and are rare and endangered, heavily relied on for industry and the running of society.
what is core charge
the attraction of the nucleus with the outer shell electrons
what is the pattern of atomic radii
atoms get bigger as we move down a group (because extra shells are used), and they get smaller from left to right (because of core charge)
how to determine nuclear charge
core charge= # of protons - # of inner shell electrons
what is the pattern of reactivity
as you go down a group of metals they get more reactive (as its easier to lose electrons)
as you go down a group of non-metals they get less reactive (as its easier to gain electrons)
what is electronegativity
the ability of an atom to attract electrons
what is first ionization energy
the amount of energy required to remove 1 electron from an atom.
what is the pattern of first ionization energy
as you go down a group the energy level decreases (due to core charge remaining the same)
left to right it increases (core charge increases and therefore electrons are attracted more to the nucleus)
