Group 1 - physical properties - Groups in the periodic table - AQA - GCSE Chemistry (Single Science) Revision - AQA - BBC Bitesize (2023)

FAQs

What are the physical properties of group 1 in the periodic table? ›

Group one elements share common characteristics. They are all soft, silver metals. Due to their low ionization energy, these metals have low melting points and are highly reactive. The reactivity of this family increases as you move down the table.

Properties of the Group 1 Elements

They are all soft metals which can easily be cut with a knife. They have relatively low densities and low melting points. They are very reactive (they only need to lose one electron to become highly stable)

Group 1A (or IA) of the periodic table are the alkali metals: hydrogen (H), lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr).

Group one element shares common characteristics. they're all soft, silver metals. because of their low ionisation energy. Group 2 elements are low density, low melting points,soft and strong in their metal states.

All the Group 1 elements are very reactive . They must be stored under oil to keep air and water away from them. When they react with water, Group 1 elements form metal hydroxides which are alkaline (with a pH above 7). This is why they are called alkali metals.

The alkali metals (group 1) are very reactive, readily form ions with a charge of 1+ to form ionic compounds that are usually soluble in water, and react vigorously with water to form hydrogen gas and a basic solution of the metal hydroxide.

The Group 1 elements have similar properties because of the electronic structure of their atoms – they all have one electron in their outer shell.

Reason: Elements in a group have the same number of electrons in the outermost shell hence they have similar chemical properties.

For example, the elements of Group 1 are known as the alkali metals, Group 2 are the alkaline earth metals, Group 17 are the halogens, and Group 18 are the noble gases.

Why is group 1 most reactive? ›

Because they have just one valence electron, group 1 elements are very reactive. As a result, they are found in nature only in combination with other elements.

Groups are numbered 1–18 from left to right. The elements in group 1 are known as the alkali metals; those in group 2 are the alkaline earth metals; those in 15 are the pnictogens; those in 16 are the chalcogens; those in 17 are the halogens; and those in 18 are the noble gases.

Physical properties. The alkali metals have the high thermal and electrical conductivity, lustre, ductility, and malleability that are characteristic of metals. Each alkali metal atom has a single electron in its outermost shell.

Like other metals, alkali metals are good conductors of heat and electricity, malleable, and ductile.

The alkali metals also have low densities . They are low enough for the first three (lithium, sodium and potassium) to float on water.

All the group 3 elements are rather soft, silvery-white metals, although their hardness increases with atomic number. They quickly tarnish in air and react with water, though their reactivity is masked by the formation of an oxide layer.

The group 1 elements react with oxygen from the air to make metal oxides . At room temperature, oxygen reacts with the surface of the metal. This forms a white oxide, which covers the surface. The metal below the surface does not react.

Alkali metals are the metals that belong to the group 1A of the periodic table. All the alkali metals have only one electron in their outermost shell (also called valency shell/ultimate shell). The alkali metals are also called as the Lithium family, named after the leading element-Lithium.

Are group 1 elements reactive? ›

Group 1 of the periodic table includes hydrogen and the alkali metals. Because they have just one valence electron, group 1 elements are very reactive. As a result, they are found in nature only in combination with other elements. Alkali metals are all solids at room temperature.

The representative elements are located in groups 1A to 7A. They are called representative elements because they display a wide range of physical and chemical properties.

Periodic Table of Elements. The elements in groups 1, 2, and 13 to 18 are called representative elements.

Group 1: Alkali Metals

Group 1 elements are called alkali metals because of their ability to displace H₂(g) from water and create a basic solution. Alkali metals are also known to react violently and explosively with water. This is because enough heat is given off during the exothermic reaction to ignite the H₂(g).

Elements of group 1 are known as alkali metals. They have 1 valence electron. In order to be stable they lose this electron and gets themselves oxidized. Hence, they are good reducing agents.

All elements in group 1 are known as the alkali metals. They all have one electron in their outer shell which they need to lose to achieve stability. This means that they all share similarities in their chemical and physical properties.

The group 1 and 2 differ from each other depending on the number of electrons in their outermost orbital. The key difference between group 1 and group 2 elements is that all group 1 elements have unpaired electrons in their outermost orbital, whereas group 2 elements have paired electrons in their outermost orbital.

Alkali metals are among the most reactive metals. This is due in part to their larger atomic radii and low ionization energies. They tend to donate their electrons in reactions and have an oxidation state of +1.

So, Cesium is the most reactive element in group IA. Note: All the alkali metals react vigorously with halogens to produce salts, as the halogens needs one electron to complete its octet and alkali metals can readily lose electrons to have an oxidation state of +1.

The reactivity of group 1 elements increases as you go down the group because: the atoms become larger. the outer electron becomes further from the nucleus. the force of attraction between the nucleus and the outer electron decreases.

How many elements are in group 1? ›

Alkali Metals, series of six chemical elements in group IA of the periodic table in order of their increasing atomic number are lithium Li, sodium Na, potassium K, rubidium Rb, cesium Cs, and francium Fr.

Group 1 will have only one unpaired electron with one electron in its valence shell making atom donate electron to get octet configuration so called metals and alkali in nature. Hence, group 1 elements are called alkali metals.

Group 1 compounds are more stable to heat than the corresponding compounds in Group 2. You will often find that the lithium compounds behave similarly to Group 2 compounds, but the rest of Group 1 are in some way different.

Alkali metals have large atomic radii between neighboring atoms of group 1 and show a weaker force of attraction due to which they are generally soft and thus have a low melting point.

Solution: In both the group 1 and 17: metallic character increases down the group, atomic radii increases as the atomic number increases and electronegativity decreases on moving down a group.

Lithium, sodium and potassium are all less dense than water, and so float on water. Rubidium and caesium are both a bit denser than water, and so sink in water.

All the alkali metals react vigorously with cold water. In each reaction, hydrogen gas is given off and the metal hydroxide is produced. The speed and violence of the reaction increases as you go down the group. This shows that the reactivity of the alkali metals increases as you go down Group 1.

As with all metals, the alkali metals are malleable, ductile, and are good conductors of heat and electricity. The alkali metals are softer than most other metals. Cesium and francium are the most reactive elements in this group. Alkali metals can explode if they are exposed to water.

Trends in Density

The metals in this series are relatively light—​lithium, sodium, and potassium are less dense than water (less than 1 g cm^-3).

Are group 1 elements heavy or light? ›

The elements are heavy metals since their atomic size is large. The energy binding atoms are high hence the elements have a high melting point. The melting points of elements decrease down the sub group. The electropositive character increases down the sub group and the elements are strong oxidizing agents.

Alkali metal (Group IA) compounds are soluble.

Physical properties. The alkali metals have the high thermal and electrical conductivity, lustre, ductility, and malleability that are characteristic of metals. Each alkali metal atom has a single electron in its outermost shell.

Group 1 elements are very reactive, because they readily give up their one valence electron in order to form a noble gas structure. Group 1 elements are able to form sodium hydroxide, sodium carbonate, sodium bicarbonate, and sodium thiosulfate.

Atoms of group 1 elements all have one electron in their outer shell. This means that the alkali metals all have similar chemical properties .

The elements that are generally good conductors of electricity belong to the following groups on the periodic table: Group 1: The alkali metals, such as lithium, sodium, and potassium, are highly conductive. Group 2: The alkaline earth metals, such as beryllium, magnesium, and calcium, are also good conductors.

This is why the group 1 metals are known as the alkali metals. As can be seen by the equations for the reactions, all of the alkali metals react with, and dissolve into, water to form strongly alkaline solutions of metal hydroxides and hydrogen gas.

Elements of group 1 are known as alkali metals. They have 1 valence electron. In order to be stable they lose this electron and gets themselves oxidized. Hence, they are good reducing agents.

Group 1 of the periodic table includes hydrogen and the alkali metals. Because they have just one valence electron, group 1 elements are very reactive. As a result, they are found in nature only in combination with other elements.

Transition metals are much stronger, denser and harder than the group 1 elements. Their melting points are also much higher. For example, titanium melts at 1,668 ^oC, compared to potassium which melts at 63.5 ^oC. However, the transition metals are less reactive than the group 1 alkali metals.