Why do elements in the same group have similar physical and chemical properties

Electronic structures and the periodic table The electronic structure of an element is linked to its position on the periodic table . Feature Link Number of shells Period number Number of electrons in outermost shell Group number Numbers added together Atomic number The electronic structure of sodium (2.8.1) shows that sodium, Na: • is in period 3 • is in group 1 • has an atomic number of (2 + 8 + 1) = 11 Note that there are some exceptions to the pattern shown with the example above. Exception Reason Hydrogen Has only 1 electron but not placed in group 1 as it does not share properties with the rest of the group - it is placed by itself on the periodic table Helium, neon and other elements in this group These elements have full outer shells - helium is 2, neon is 2.8, argon is 2.8.8, and their group number is group 0 Electronic structures and properties of elements The electronic structures of atoms help explain the properties of elements and the structure of the periodic table. When atoms collide and react, it is the outer electrons that meet and interact. So, elements in the same group have similar chemical properties because they have the same number of electrons in their outer shell. The electronic structures of the elements in group 1: The atoms of all group 1 elements have similar chemical properties and reactions because they all have one electron in their outer shell. Similarly, the atoms of all group 7 elements have similar chemical properties and reactions to ea...

Table of Contents • • • • Why do elements belong to the same group have similar chemical properties? In a group, the elements having same number of valence electrons are out together. Hence the chemical properties of the elements in a group are similar. In a group of the periodic table, all the elements have the same number of valence electrons therefore their chemical properties are similar. What do elements with similar chemical properties have in common? The vertical columns on the periodic table are called groups or families because of their similar chemical behavior. All the members of a family of elements have the same number of valence electrons and similar chemical properties. Which elements are most likely to have similar chemical properties? Sodium and potassium share similar physical and chemical properties because they are in the same family or group called Alkali metals. Both will have the same valence electrons and they are both very reactive. What is the property which is similar to the elements of the same period? All elements in a row have the same number of electron shells. Each next element in a period has one more proton and is less metallic than its predecessor. Arranged this way, groups of elements in the same column have similar chemical and physical properties, reflecting the periodic law. What elements that have the same properties? Two different elements have similar chemical properties when they have the same number of valence electrons in their ...

24 What is physical property in chemistry? Why do elements in the same group have similar physical and? Each element within a group has similar physical or chemical properties because of its atom’s outermost electron shell (most chemical properties are dominated by the orbital location of the outermost electron). What do elements in the same group have in common? The elements in each group have the same number of valence electrons. As a result, elements in the same group often display similar properties and reactivity. Which elements have similar physical properties? The answer is b. Elements in the same group have the same number of valence electrons and so interact with other elements in a similar way. They display similar physical and chemical properties. For example, the halogens (F, Cl, Br, I) all react similarly. Why do elements in the same group have similar properties quizlet? Elements in the same family have similar properties because they have the same number of valence electrons. How do you know if elements have similar properties? Two different elements are likely to have similar chemical properties when they have the same number of valence electrons. Elements with the same number of valence electrons are found in the same column of the Periodic Table. Elements with the same valence shell are found in the same row on the Periodic Table. What determines physical properties of an element? All elements have differing physical properties depending on their bonding ...

\( \newcommand\) • • • ⚙️Learning Objectives • To distinguish physical from chemical properties. All matter has physical and chemical properties. Physical properties are characteristics that scientists can measure without changing the composition of the sample under study, such as mass, color, and volume (the amount of space occupied by a sample). Chemical properties describe the characteristic ability of a substance to react to form new substances; they include its flammability and susceptibility to corrosion. All samples of a pure substance have the same chemical and physical properties. For example, pure copper is always a reddish-brown solid (a physical property) and always dissolves in dilute nitric acid to produce a blue solution and a brown gas (a chemical property). Physical Property A physical property is a characteristic of a substance that can be observed or measured without changing the identity of the substance. Silver is a shiny metal that conducts electricity very well. It can be molded into thin sheets, a property called malleability. Salt is dull and brittle and conducts electricity when it has been dissolved into water, which it does quite easily. Physical properties of matter include color, hardness, malleability, solubility, electrical conductivity, density, melting points, and boiling points. For the elements, color does not vary much from one element to the next. The vast majority of elements are colorless, silver, or gray. Some elements do have disti...

\( \newcommand\) • • • • • • • • • • • • • • • • Properties of elements generally show a periodic trend that correlates with their position in the periodic table. The properties and their periodic trends are described below. Periodic trend of valence electrons All elements in a group have the same number of valence electrons equal to the first digit of their group number. For example, 1st group of hydrogen and alkali metals has one valence electron, 2nd group of alkali metals has two valence electrons, halogens in 17th group have seven valence electrons, and noble gases in 18th group have eight valence electrons. Caution The transition metals in groups 3 to 12, and inner-transition metals, i.e., lanthanoids and actinoids -the two rows of elements placed below the periodic table, are the exception to the general trend of valence electrons described above. Valence electron configurations of transition metals and inner-transition metals are not described here; it is beyond the scope of this book. The valence electrons mainly determine the chemical properties of the elements. The elements in the same group have similar chemical properties because they have the same valence shell electron configuration. The elements in a row show a gradual change in chemical properties because their valence shell electron configuration changes gradually along the row. Lewis symbols • Lewis symbols show the valence electrons as dots around the symbol of an element. One dot represents one valence...

\( \newcommand\) • • • • • • • • • • • • • • The elements within the same group of the periodic table tend to exhibit similar physical and chemical properties. Four major factors affect reactivity of metals: nuclear charge, atomic radius, shielding effect and sublevel arrangement (of electrons). Metal reactivity relates to ability to lose electrons (oxidize), form basic hydroxides, form ionic compounds with non-metals. In general, the bigger the atom, the greater the ability to lose electrons. The greater the shielding, the greater the ability to lose electrons. Therefore, metallic character increases going down the table, and decreases going across -- so the most active metal is towards the left and down. Group 1: The Alkali Metals The word "alkali" is derived from an Arabic word meaning "ashes". Many sodium and potassium compounds were isolated from wood ashes (\(\ce \nonumber \] Colors via Absorption The color of a chemical is produced when a valence electron in an atom is excited from one energy level to another by visible radiation. In this case, the particular frequency of light that excites the electron is absorbed. Thus, the remaining light that you see is white light devoid of one or more wavelengths (thus appearing colored). Alkali metals, having lost their outermost electrons, have no electrons that can be excited by visible radiation. Alkali metal salts and their aqueous solution are colorless unless they contain a colored anion. Colors via Emission When alkali...

The repeating sequence of physical and chemical properties among the elements, when they were listed in order of increasing atomic mass, was what led to the creation of the Periodic Table of the Elements. Today's Periodic Table is arranged in order of increasing number of protons in the nuclei of the atoms of the elements, with the elements aligned so that those with similar properties are in the same column, or group. It is actually the electrons, not the protons, that give rise to the properties that repeat from period to period, but since a neutral atom has the same number of electrons as protons, listing the elements by atomic number works just fine. We now know that electrons are arranged around the atomic nucleus in a structured arrangement, and it is the outermost electrons, called the valence electrons, that are mainly responsible for interacting with other atoms, and thus are responsible for both physical and chemical properties. Being very small, electrons have significant wave nature, so their behavior cannot be adequately represented by classical physics, but can be described by quantum mechanics. The derivation is complicated but says that electrons around a nucleus can exist only in certain states identified by their quantum numbers n, l, and m. These states have probability distributions in space that we visualize as shapes, called orbitals. At most two electrons with different values of a fourth quantum number, s, can "occupy" the same shape, or orbital. Th...