The periodic table Flashcards
What are some properties of group 1 Alkali metals
Soft
Highly reactive
Low melting points
Form soluble salts
Where are the d - block elements
3-12
What are non - metal properties
poor conductors
not hard
solid , liquid or gas at room temperature
At room temperature what are florine and chlorine
Gasses
At room temperature what is Br
liquid
At room temperature what is I
solid
What are the properties of the Noble gasses
Highly reactive
Gases
What is the first row of the f-block called
Lanthanides
What is the second row of the f-block called
Actinides
What are the properties of f-block
Complex and heavy metals
Highly reactive
High melting and boiling points
Elements in the same period have the same number of
shells
Across a period
Charge of nucleus …
Atomic Radius …
Increases
Decreases
Where are the metals and non-metals located
metals - left
non metals - right
Definition of Ionisation Energy
The energy needed to remove one mol of an electron from a mole of gaseous atoms of ions
Atomic radius and Ionisation Energy are
Inversely Proportional
What happens down a group between
Atomic radius :
Ionisation Energy :
Increases
Decrease
What happens across a period between
Atomic Radius
Ionisation Energy
Decrease
Increase
Define electron affinity
The energy released when one mole of an atom gains an electron to form a negatively charged ion
Explain the trend between electron affinity down the group
decreases
Explain the trend between electron affinity across a period
increases
Define Electronegativity
The ability of an atom to attract a pair of bonded electrons
Electronegativity decreases down a group because
nuclear charge increases
increased shielding
large atomic radius due to increase in electron shell
Electronegativity increased across a period because
Effective nuclear charge increases
Stronger attraction between the nucleus and the shared pair of electrons
What decreases as you go down group 1
ionisation energy
What increases as you go down group 1
reactivity
number of occupied energy levels
What increases down group 17
number of occupied energy levels
What decreases down group 17
electron affinity
reactivity
Define first ionisation energy
minimum energy required to lose one mole of electrons from one mole of gaseous atoms to produce one mole of gaseous ions
Explain why the first ionisation energy decreases down a group (3)
• Going down a group atomic radii increases and electrons occupy higher energy levels
• Electrons in higher energy levels have a weaker attraction to the nucleus.
• Less energy is required in order to remove an electron
Explain why first ionisation energy increases across a period
Going across there are more protons in the nucleus and more electrons occupying the outermost energy level (effective nuclear charge)
• A greater number of electrons in the outermost energy level results in a stronger attraction to the nucleus
• More energy is required in order to remove an electron
Atomic radius
Increases down a group
decreases across a period
Define First Electron affinity
the amount of energy released when a neutral atom gains an electron to form a negatively charged ion
Why does First electron affinity decrease down a group
The atomic radius becomes larger , the attraction for an additional electron is less , since the effective nuclear charge is reduce due to increased shielding
Why does electron affinity increase across a period
Elements across a period have a higher effective nuclear charge.
Stronger attraction between the added electron and the nucleus
What are the 6 characteristic properties of transition elements
• Variable oxidation states
• High melting points
• Magnetic properties
• Catalytic properties
• Formation of coloured compounds
• Formation of complex ions
if the ionisation number is 2+ what its oxidation number
+2
What is a transition element
element with a partially filled d-subshell
what is effective nuclear charge
more electrons in shells
What type of metals have low EA
metals
What type of metals have a high EA
non-metals
Why do metals have low electronegativities
because they lose electrons easily
why do non-metals have high electronegativities
as they gain electrons to fill their outer shell
What is the trend in melting points ?
Increase across a period until group 14 then decrease
What is the trend in metallic character
Increases down a group
Decreases across a period
What is the acidic state of sodium oxide Na2O
Basic
What is the acidic state of magnesium oxide Mgo
Basic
What is the acidic state of Aluminium Oxide Al2O3
Amphoteric
What is the acidic state of Silicon Oxide SiO2
acidic
What is the acidic state of Phosphorus
Acidic
What is the acidic state of sulfur oxide SO2
acidic
What is the acidic state of chlorine oxide
Acidic
