Periodic Table Flashcards
Define periodic property
A physical or chemical property that is repeated in a regular pattern for elements when they are arranged according to their atomic number
Define period
Refer to the rows in the periodic table. Drone left to right in the table the elements change from metals to non metals
Define group
Refer to the columns in the periodic table. Elements in a given group bear many similar physical and chemical properties
What are the periodic properties
Atomic size or radius, ionization energy, electron affinity and electronegativity
Define atomic size or radius
A measure of the size of the atom. It is found by determining half of the separation distance between the nuclei of the two adjacent atoms
What are the trends of atomic size or radius
Increases down each group because he valence electrons occupy an energy level that is farther from the nucleus.
Decreases across a period because the positive charge in the nucleus increases across a period
Define ionization energy
The energy needed to remove the most loosely held electron from the atom
What are the trends of ionization energy
Decrease down a group
Increase across a period
Define electron affinity
A measure of energy change that occupies when an electron is added to the outer energy level of an atom to form a negative ion on anion
What are the trends or electron affinity
Decreases down a group
Increases across a period
Define electronegativity
Measure of and atoms ability to attract electrons in a chemical bond
Now recorded for noble gases because they do not usually participate in bonding
What are the trends of electronegativity
Increases across a period
Decreases down a period
What is the chemical reactivity of alkali metals
Increases as you go down the group Each metal gives a distinct colour flame in the flame test Relatively hard but hardness decreases as you go down the group Low density (some float on water)
What is alkali reactivity with water
Very reactive
Generates hydrogen gas and aqueous solution of metal hydroxide
What is alkali reactivity with oxygen
Very reactive with oxygen
Reacts with oxygen to form an oxide
Alkali earth metals chemical reactivity
Less reactive in water than alkali but more then regular metals
Form ionic compounds with non- metals
All burn in air to form oxides
Oxides of these metals react with water to form metal hydroxide solutions
Physical properties of alkali earth metals
Harder and denser than alkali metal (decreases as you go down)
Higher melting point and higher boiling point than alkali metals(decreases as you go down)
Describe group IIIa
Metals
None of the elements in this group react with air or water at room temperature
Group IVa
Contains non-metal carbon
Group Va
Contains the non metal nitrogen
group VIa
Contains oxygen and sulfur
Can for ionic compounds w metals
Can form covalent compounds with non metallic elements like hydrogen
Oxygen reacts with most other elements to form oxides
Transitional metals
Topical metals Good conductors of heat and electricity Malleable Ductile Higher melting and boiling point and harder tougher and stronger than alkali metals but less reactive
Semi metals
Have some but not all the properties of metals Good semi conductor Very high melting and boiling point Very hard Form giant covalent structures
Halogens reactivity
Increases as you go up the group
Most reactive non metal
React w alkali metals to form salts
Halogens physical properties
Coloured non metals State varies Low melting and boiling point but decreases down the group Brittle when solid Poor conductors
Noble gasses
Colour less
Low melting and boiling point
Individual atoms
Unreactive
Physical properties of metal
Shiny metallic appearance Solid at room temperature High melting and boiling point malleable Ductile Conduct heat and electricity High density Most are hard
Chemical properties of a metal
React with air or oxygen to form oxides
Form basic oxides that react with acids to form salts and hydrogen gas
Metals readily form positive ions in compounds by losing electrons
Their oxides and chlorides are usually ionic in terms of chemical bonding
Metal oxides
Metals react with oxygen to form basic oxides
Basic because they reacts with water to form alkaline solutions which react with acids to form salts
Some do not react in water because they do not form hydroxides
Tend to be ionic in bonding character with high melting points
Activity series of metals
The higher the metal in the series the more reactive it is the more reactive a metal is the harder it is to extract it from the ore the more reactive a metal the more susceptible it is to corrosion from oxygen and water
Physical properties of non metals
Vary in state
Solid non metals are generally brutal and lack metallic luster
Most are poor conductor of electricity and heat
(Except carbon graphite)
Low melting point
Low density
Chemical properties of non metals
For acidic oxides when burned in air or oxygen
Do not usually react with acids
Non metal oxides
Are acidic
React with water to for acids
Have low melting/ boiling points
