Chemistry Level 10 Pack

Compounds formed when Group 1 metals react with water, producing a metal hydroxide (e.g., sodium hydroxide, NaOH) and hydrogen gas.

A reaction that releases heat.

The ability of a substance to act as a base.

Group 1 metal hydroxides dissolved in water, making the solution basic.

The type of bonding where electrons are free to move throughout the structure, found in metals.

A characteristic of Group 1 metals, where they are soft and can be cut with a knife.

Storing alkali metals in oil to prevent them from reacting with moisture or oxygen in the air.

A measure of how easily a substance can be drawn into wires.

Group 1 elements are called alkali metals because they react with water to form alkaline solutions, which are solutions with a pH greater than 7.

The reactivity of Group 1 metals increases as you move down the group. This is because the outermost electron is further away from the nucleus and easier to remove.

As you move down the group, the attraction between the nucleus and the outermost electron decreases. This leads to a larger atomic radius.

Sodium reacts vigorously with water, releasing heat and producing hydrogen gas and sodium hydroxide. Potassium reacts even more vigorously, producing a flame and exploding.

The first three metals in Group 1 are lithium (Li), Sodium (Na) and Potassium (K) . Their electron configuration is [He]2s1, [Ne]3s1 , and [Ar]4s1 respectively.

Group 1 elements have low melting and boiling points because the weak metallic bonds between their atoms are easily broken.

Group 1 elements tend to form +1 ions because they only have one valence electron, which they readily lose to achieve a stable octet configuration.

The energy needed to lose the valence electron decreases as you move down the group. This is because the outermost electron is farther from the nucleus and easier to remove.

Elements in Group 2 of the periodic table, known for their reactivity and tendency to form +2 ions.

The process of adding heat to a substance to change its state from solid to liquid.

The amount of energy required for a substance to transition from its solid state to its liquid state.

The tendency of a substance to dissolve in a solvent, usually water.

The reaction of an element with oxygen, often resulting in the formation of an oxide.

The tendency of an element to lose or gain electrons, determining its ability to form chemical bonds.

The distance from the nucleus to the outermost electron shell in an atom.

A series of chemical steps to determine the identity of an element by observing the color of its flame.

Alkaline earth metals are the elements found in group 2 of the periodic table. They share common chemical properties and characteristic reactions with oxygen, water, and acids.

Alkaline earth metals are known for their reactivity, which increases as you move down the group. This means they react more readily with other substances, like oxygen and water.

Alkaline earth metals react with oxygen to form metal oxides. For example, magnesium reacts with oxygen to form magnesium oxide.

The reaction of alkaline earth metals with water produces a metal hydroxide and hydrogen gas. For example, calcium reacts with water to form calcium hydroxide and hydrogen gas.

Alkaline earth metals react with acids to form a salt and hydrogen gas. The reactivity increases as you progress down the group.

The physical properties of alkaline earth metals change down the group. Their melting and boiling points decrease, density increases, and reactivity with water increases.

The increase in reactivity down the group is due to the increasing atomic radius. The outer electron becomes easier to remove, making the element more reactive.

Alkaline earth metals are found in abundance in the Earth's crust, making them crucial components of various minerals and rocks.

The amount of dissolved calcium and magnesium ions present in water.

A layer of calcium or magnesium compounds that forms on the inside of appliances like water heaters and boilers.

Scale acts as an insulator, causing water heaters and boilers to work harder to heat water, resulting in higher energy consumption and increased costs.

Hard water leaves a residue on skin and hair, causing dryness, irritation, and an unclean feeling.

The formation of soap scum and scale requires more cleaning products and effort to achieve cleanliness.

A test used to determine the hardness of water by observing how well soap lathers.

The reaction of soap (sodium stearate) with calcium ions in hard water produces an insoluble compound called calcium stearate, which forms soap scum.

Soap lathers easily in soft water because there are fewer calcium and magnesium ions to react with.

Hard, strong, and dense metals that excel at conducting heat and electricity. They also have very high melting points.

The ability of a transition metal atom to lose a varying number of electrons, depending on its chemical environment. This leads to different oxidation states or valences.

Transition metals can form compounds with different colors, resulting in a diverse range of hues.

Transition metals often act as catalysts, speeding up chemical reactions without being consumed themselves.

A transition metal with an oxidation state of +2 is written in roman numerals like 'Iron (II)' to differentiate it from other oxidation states.

The reaction between iron and steam, where iron reacts with water vapor to form iron oxide (rust) and hydrogen gas.

The reaction between iron and hydrochloric acid, where iron reacts with the acid to form iron chloride and hydrogen gas.

The reaction between iron and chlorine gas, where iron reacts with chlorine to form iron chloride.