Chapter 5 Flashcards
How many electrons fill shell number 1?
2
How many electrons fill shell number 2?
8
How many electrons fill shell number 3?
18
How many electrons fill shell number 4?
32
What are shells regarded as?
energy levels
As the shell number increases, does energy increase or decrease?
increase
What is the principal quantum number, n?
shell number/energy level number
number of electrons =
2n²
What are shells made up of?
atomic orbitals
What is an atomic orbital?
1) region around the nucleus that can hold up to two electrons, with opposite spins
2) region in space where there is a high probability of finding an electron
What are the different types of orbitals?
1) s
2) p
3) d
4) f
Do each type of orbitals have the same or different shape?
different
In a s-orbital what shape is the electron cloud?
sphere
How many s-orbitals does each shell from n=1 contain?
1
In a s-orbital, the greater the shell number n, the…
greater the radius
In a p-orbital what shape is the electron cloud?
dumb-bell
How many electrons can an orbital hold?
1 or 2
How many p-orbitals does each shell from n=1 contain?
3
What angle are p-orbitals to one another?
right angles
With a p-orbital, the greater the shell number n, the…
further the o-orbital is from the nucleus
How many d-orbitals does each shell from n=1 contain?
5
How many f-orbitals does each shell from n=1 contain?
7
What charge do electrons have?
negative
Do electrons attract or repel each other?
repel
Which direction are electron spins?
up or down
Do the two electrons in an orbital have the same or opposite spins?
opposite
Why do the two electrons in an orbital have opposite spins?
to counteract the repulsion between the negative charges of the two electrons
How can electron configurations be expressed more simply?
1) previous noble gas in the periodic table
2) outer shell electrons
What are cations?
positive ions that are formed when atoms lose electrons
What are anions?
negative ions formed when atoms gain electrons
What is a s-block element?
highest energy electrons in s-sub-shell
What is a p-block element?
highest energy electron in p-sub-shell
What is a d-block element?
highest energy electron in d-sub-shell
What is ionic bonding?
the electrostatic attraction between positive + negative ions
What state are ionic compounds in at room temperature?
solid
Why are ionic compounds solid at room temperature?
there is insufficient energy to overcome strong electrostatic forces of attraction between oppositely charged ions in giant ionic lattice
Do ionic compounds have low or high melting and boiling points?
high
What are the two main processes of solubility?
1) ionic lattice broken down
2) water molecules attract + surround ions
When do ionic compounds conduct electricity?
1) once melted
2) once dissolved in water
Why do ionic compounds not conduct electricity in the solid state?
1) ions in fixed position in giant ionic lattice
2) no mobile charge carriers
Why do ionic compounds conduct electricity when liquid or dissolved in water?
1) solid ionic lattice breaks down
2) ions free to move as mobile charge carriers
What is covalent bonding?
1) strong electrostatic attraction between a shared pair of electrons and nuclei of bonded atoms
2) overlap of atomic orbitals, each containing 1 electron, to give shared pair of electrons
Between which atoms does covalent bonding occur?
1) non-metallic elements
2) compounds of non-metallic elements
3) polyatomic ions
What are lone pairs?
paired electrons that are not shared
What is a dative covalent/coordinate bond?
covalent bond in which shared pair of electrons is supplied by one bonding atom only
What does average bond enthalpy measure?
covalent bond strength
