ions, properties of metals, reactivity of metals, molecules compounds and elements Flashcards
(28 cards)
Why are the outer shell electrons important?
Because they are the electrons involved in forming bonds with other atoms to achieve a stable electron. They also determine the atom’s chemical properties.
How do the valence electrons influence reactivity?
Atoms are most stable when they have a full outer shell, so if it is not full, then the atom tries to quickly get rid of it or gain electrons, making it more reactive.
What is a neutral atom?
An atom that has equal protons and electrons.
What is a cation?
An atom that has lost electrons, giving it a positive charge.
What is an anion?
An atom that gains electrons, giving it a negative charge.
How are ions formed?
When an atom gains or loses electrons and becomes charged.
Why do metals seem to form cations and non-metals seem to form anions?
Because metals have a tendency to lose electrons to achieve a stable electron configuration, while nonmetals have a tendency to gain electrons to achieve a stable electron configuration.
How do you determine the symbol and charge of ions?
A cation always has a + symbol in front of the number of valence electrons lost. An anion always has a - symbol in front of the number of electrons gained.
What charge is a cation?
Positive.
What charge is an anion?
Negative.
What is metallic bonding?
Metal ions forming a lattice structure in a sea of delocalised electrons.
What are the main properties of metals?
Good conductors of electricity and heat, strong, ductile and shiny/lustre
Why do properties of metals make them ideal for various uses?
Makes them suitable for construction and transportation to electronics.
What is the arrangement of atoms in metals?
Lattice structure (a sea of electrons surrounding positively charged ions).
What is a metal alloy?
A substance created by combining two or more chemical elements, where at least one is a metal.
What is a metalloid?
Chemical elements whose physical and chemical properties fall in between the metal and non-metal categories.
Examples of metalloid?
Boron, silicon, arsenic.
Compare and explain the reactivity of different metals.
Group 1 metals are highly reactive (gold and silver not so reactive).
Why do we need to understand the reactivity of metals?
So we can control the process of corrosion (rusting) and use the right metals as materials in construction.
What is the trend of chemical reactivity in the periodic table?
Reactivity of metals decreases across a period (L-R) because of the less amount of valence electrons. Reactivity of metals increases when going down a group because valence electrons are easier to lose due to the larger atomic number.
Which metals react most strongly with acids?
Potassium, sodium, and lithium.
What is the worded equation layout for metal and acid reaction?
Metal + acid → ionic compound + hydrogen gas.
What are the ionic compounds for different acids?
Hydrochloric acid = chloride, sulfuric acid = sulfate, phosphoric acid = phosphate.
Provide an example of a metal reacting with hydrochloric acid.
Lithium + hydrochloric acid → lithium chloride + hydrogen gas.
