Periodic Table Flashcards
What are the factors affecting atomic radius?
- number of filled quantum shells
- nuclear charge
- shielding effect
How does number of filled principal quantum shell affect atomic radius?
The greater the number of filled principal quantum shells, the further the valence electrons are from the nucleus, the larger the atomic radius
How does nuclear charge affect atomic radius?
The greater the nuclear charge the stronger the electrostatic attraction the nucleus has on valence electrons
What affects shielding effect?
The larger the number of filled inner principal quantum shells of electrons, the greater the shielding effect experienced by valence electrons
What is the trend of atomic radius across a period?
- across a period, atomic radii of elements decrease gradually
- there is an increase in nuclear charge while shielding effect by inner principal quantum shells of electrons remains relatively constant, thus nuclear charge increases
What is the trend of atomic radii down a group?
- down a group, atomic radii of elements increase gradually
- down the group, the number of filled principal quantum shells increases, the increase in nuclear charge is cancelled out by the increase in shielding effect by the inner principal quantum shell of electrons
How do cationic radii compare with atomic radii and why?
- cationic radii is always smaller than atomic radii
- atoms lose electrons to form cations, thus cations formed usually have one less principal quantum shell of electrons
How do anionic radii compare with atomic radii and why?
- anionic radii is always larger than atomic radii
- to form anions, electrons are added to the outermost principal quantum shell of atoms, as a result, there is greater electron-electron repulsion in the outermost principal quantum shell of anions formed
What is the trend of ionic radii of isoelectronic ions with increasing atomic number?
- isoelectronic radii of isoelectronic ions decrease with increasing atomic number
- as atomic number increases, nuclear charge increases, ionic radii decreases
What is the variation of electrical conductivities across period 3?
- electrical conductivities are high for Na, Mg and Al and increases from Na to Al
- Na, Mg and Al have giant metallic lattice structure
- number of delocalised valence electrons increases from Na to Al
- electrical conductivity drops sharply at Si
- Si has a giant covalent structure and is a semi conductor
- electrical conductivities drop to 0 at P₄ and remains at zero to Ar
- P₄ to Cl₂ have simple covalent structures and Ar has a monoatomic structure
- there are no mobile charge carriers to conduct electricity
What is the variation of electrical conductivities across period 2?
- electrical conductivities are high for metals Li and Be and increases from Li to Be
* Li and Be has giant metallic lattice structure
* number of delocalised valence electrons increases from Li to Be - electrical conductivities drop sharply to zero at B and remains at 0 from B to Ne except for C (graphite)
* B and C (diamond) have giant covalent structures, N₂ to F₂ have simple covalent structures and Ne has a monoatomic structure
* no mobile charge carriers to conduct electricity
* C (graphite) has delocalised valence electrons along the layers to conduct electricity in the direction parallel to the layers
What are the trends for melting point and ΔHfᵤₛ of period 3 elements?
- melting points of Na, Mg and Al are fairly high and increases from Na, Mg to Al
* Na, Mg and Al have giant metallic lattice structures
* a large amount of energy is required to overcome the strong electrostatic forces of attraction between metal cations and sea of delocalised mobile valence elctrons
* as number of delocalised valence elecrtons increases from Na to Al, strength of metallic bonds increases - melting point reaches a maximum at Si
* Si has a giant covalent structure with strong and extensive covalent bonds between Si atoms - melting point drops sharply to P and melting point remains low fro P to Ar
* phosphorous, sulfure and chlorine have simple covalent structures and Ar has a monoatomic structure
* a smaller amount of energy is required to overcome the weak id-id
* melting point of sulfur, phosphorous, chlorine, argon
* S₈, P₄, Cl₂
* number of electrons of S₈ > P₄ > Cl₂, strength of id-id S₈ > P₄ > Cl₂
What are the trends for melting point and ΔHfᵤₛ of period 2 elements?
- melting point of Li and Be are fairly high and increases from Li to Be
* Li and Be have giant metallic lattice structures with strong electrostatic forces fo attraction between metal cations and sea of delocalised mobile valence electrons
* as number of delocalised mobile valence increases from Li to Be, strength of metallic bonds increases - melting point continues to increase from B and reaches a maximum at C
* B and C have giant covalent structures with strong covalent bonds between atoms - melting point drops sharply to N and remains low from N to Ne
* N, O and F have simple covalent structures while Ne have monoatomic structure, with weak id-id
* a small amount of energy is required to overcome the weak id-id
What is enthalpy change of fusion, ΔHfᵤₛ?
Enthalpy change when 1 mole of substance changes from solid to liquid
What is enthalpy change of vaporisation, ΔH(vap)?
enthalpy change when 1 mole of substance changes from liquid to gas
What is the structure of Li?
Giant metallic lattice structure
What is the structure of Be?
Giant metallic lattice structure
What is the structure of Boron?
giant covalent
What is the structure of C?
giant covalent
What is the hybridisation for C atoms in diamond?
sp³ hybridised
What is the hybridisation of C in graphite?
- sp2 hybridised
- 4th 2p electron of each carbon atom is delocalised along the layers
What is the structure of nitrogen?
Simple covalent
What is the structure of oxygen?
Simple covalent
What is the structure of fluorine?
Simple covalent