You are watching: Why do elements in the same group have similar properties
Key PointsThe physical properties of aspects depend in component on their valence electron configurations. As this configuration stays the very same within a team, physical properties tfinish to remajor somewhat constant.The most noteworthy within-group transforms in physical properties take place in Groups 13, 14, and 15, where the elements at the height are non-metallic, while the elements at the bottom are metals.The patterns in boiling and melting points vary from group to team, based on the kind of non-bonding interactions holding the atoms together.
TermsductileCapable of being pulled or extended into thin wire by mechanical pressure without breaking.physical propertyAny building that is measurable whose worth describes a physical system’s state.malleableAble to be hammered into thin sheets; qualified of being extfinished or shaped by beating with a hammer or by the pressure of rollers.
In chemistry, a group is a vertical column in the periodic table of the chemical aspects. Tright here are 18 teams in the standard regular table, including the d-block elements however excluding the f-block elements. Each element within a team has comparable physical or chemical properties because of its atom’s outermost electron shell (the majority of chemical properties are overcame by the orbital area of the outermany electron).
Common Physical Properties
A physical building of a pure substance deserve to be characterized as anything that have the right to be observed without the identity of the substance transforming. The observations generally consist of some kind of numerical measurement, although periodically tright here is a more qualitative (non-numerical) description of the residential property. Physical properties incorporate such points as:ColorBrittlenessMalleabilityDuctilityElectrical conductivityDensityMagnetismHardnessAtomic numberSpecific heatHeat of vaporizationHeat of fusionCrystalline configurationMelting temperatureBoiling temperatureHeat conductivityVapor pressureTendency to disfix in assorted liquids
These are only a few of the measurable physical properties.
Within a group of the routine table, each aspect has the same valence electron configuration. For example, lithium, sodium, potassium, rubidium, cesium, and also francium all have actually a single electron in an s orbital, whereas eextremely facet in the team including fluorine has the valence electron configuration ns2np5, wright here n is the period. This suggests the aspects of a group often exhilittle bit equivalent chemical reactivity, and also tbelow may be similarities in physical properties also.
Boiling and Melting Points
Before a conversation of the melting points of miscellaneous elements, it should be listed that some elements exist in different forms. For example, pure carbon deserve to exist as diamond, which has a really high melting point, or as graphite, whose melting point is still high however a lot lower than that of diamond.
Different teams exhilittle bit various fads in boiling and also melting points. For Groups 1 and 2, the boiling and also melting points decrease as you relocate down the group. For the shift metals, boiling and melting points mainly increase as you move down the group, yet they decrease for the zinc family. In the main team facets, the boron and carbon family members (Groups 13 and 14) decrease in their boiling and melting points as you relocate down the group, whereas the nitrogen, oxygen, and also fluorine families (Groups 15, 16, and also 17) tfinish to boost in both. The noble gases (Group 18) decrease in their boiling and also melting points down the group.
These phenomena can be construed in relation to the kinds of forces holding the aspects together. For metallic species, the metallic bonding interaction (electron-sharing) becomes even more hard as the facets gain larger (towards the bottom of the table), bring about the forces holding them together to become weaker. As you relocate ideal alengthy the table, however, polarizability and van der Waals interactions preconquer, and as larger atoms are more polarizable, they tfinish to exhibit stronger intermolecular pressures and therefore greater melting and also boiling points.
Metallic facets are shiny, generally gray or silver in color, and conductive of warmth and also electrical power. They are malleable (have the right to be hammered right into thin sheets) and ductile (can be extended right into wires). Some steels, such as sodium, are soft and also deserve to be cut with a knife. Others, such as iron, are exceptionally tough. Non-metallic atoms are dull and also are poor conductors. They are brittle as soon as solid, and many type of are gases at STP (conventional temperature and pressure). Metals give away their valence electrons when bonding, whereas non-steels tend to take electrons.A steel and a non-MetalOn the left is sodium, an extremely metallic aspect (ductile, malleable, conducts electricity). On the best is sulfur, a very non-metallic aspect.
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Metallic character boosts from appropriate to left and from optimal to bottom on the table. Non-metallic character follows the opposite pattern. This is bereason of the other trends: ionization power, electron affinity, and electronegativity. You will alert a jagged line running through the periodic table starting in between boron and aluminum – this is the separation between metallic and also non-metallic aspects, with some facets close to the line exhibiting qualities of each. The metals are toward the left and center of the routine table, in the s, d, and also f blocks. Poor steels and metalloids (somewhat metal, rather non-metal) are in the lower left of the p block. Non-metals are on the right of the table.
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