Period 4 element

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A period 4 element is one of the chemical elements in the fourth row (or period) of the periodic table of the elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behaviour of the elements as their atomic number increases: a new row is begun when chemical behaviour begins to repeat, meaning that elements with similar behaviour fall into the same vertical columns. The fourth period contains 18 elements, beginning with potassium and ending with krypton. As a rule, period 4 elements fill their 4s shells first, then their 3d and 4p shells, in that order, however there are exceptions, such as chromium.

Properties

Every single one of these elements are stable,^[1] and many are extremely common in the earth's crust and/or core. Many of the transition metals in period 4 are incredibly strong, and therefore commonly used in industry, especially iron. Copper is one of three elements that are not silver or gray in color, along with caesium and gold. Three adjacent elements are known to be toxic, with arsenic one of the most well-known poisons, selenium being toxic to humans in large quantities, and bromine, a very toxic liquid. Many elements are essential to humans' survival, such as Calcium being what forms bones.^[2]

Periodic trends

List of elements

Chemical element			Chemical series	Electron configuration
19	K	Potassium	Alkali metal	[Ar] 4s¹
20	Ca	Calcium	Alkaline earth metal	[Ar] 4s²
21	Sc	Scandium	Transition metal	[Ar] 3d¹ 4s²
22	Ti	Titanium	Transition metal	[Ar] 3d² 4s²
23	V	Vanadium	Transition metal	[Ar] 3d³ 4s²
24	Cr	Chromium	Transition metal	[Ar] 3d⁵ 4s¹ (*)
25	Mn	Manganese	Transition metal	[Ar] 3d⁵ 4s²
26	Fe	Iron	Transition metal	[Ar] 3d⁶ 4s²
27	Co	Cobalt	Transition metal	[Ar] 3d⁷ 4s²
28	Ni	Nickel	Transition metal	[Ar] 3d⁸ 4s²
29	Cu	Copper	Transition metal	[Ar] 3d¹⁰ 4s¹ (*)
30	Zn	Zinc	Transition metal	[Ar] 3d¹⁰ 4s²
31	Ga	Gallium	Post-transition metal	[Ar] 3d¹⁰ 4s² 4p¹
32	Ge	Germanium	Metalloid	[Ar] 3d¹⁰ 4s² 4p²
33	As	Arsenic	Metalloid	[Ar] 3d¹⁰ 4s² 4p³
34	Se	Selenium	Polyatomic nonmetal	[Ar] 3d¹⁰ 4s² 4p⁴
35	Br	Bromine	Diatomic nonmetal	[Ar] 3d¹⁰ 4s² 4p⁵
36	Kr	Krypton	Noble gas	[Ar] 3d¹⁰ 4s² 4p⁶

(*) Exception to the Madelung rule

Legend for the background color

Background color shows subcategory in the metal–nonmetal range:
Metal						Metalloid	Nonmetal			Unknown chemical properties
Alkali metal	Alkaline earth metal	Lanthanide	Actinide	Transition metal	Poor metal		Polyatomic nonmetal	Diatomic nonmetal	Noble gas

s-block elements

Potassium

Potassium (K) is an alkali metal, placed under sodium and over rubidium, and is the first element of period 4.^[3] It is one of the most reactive elements in the periodic table, therefore usually only found in compounds. It tends to oxidize in air very rapidly, thus accounting for its rapid reaction with oxygen when freshly exposed to air. When freshly exposed, it is rather silvery, but it quickly begins to tarnish as it reacts with air. It is soft enough to be cut with a knife and it is the second least dense element.^[4] Potassium has a relatively low melting point; it will melt just by putting it under a small open flame.^[5] It also is less dense than water, and can, in turn, float.^[6]

Calcium

Calcium (Ca) is the second element in period 4, between potassium and scandium. An alkali earth metal, calcium is almost never found in nature due to its high reactivity with water.^[7] It has one of the most widely known and acknowledged biological roles in all animals and some plants, making up bones and teeth, and used in some applications in cells, such as signals for cellular processeses. It is regarded as the most abundant mineral in the body's mass.^[8]

d-block elements

Scandium

Scandium (Sc) is the third element in period 4, between calcium and titanium, and is the first transition metal in the periodic table. Scandium is quite common in nature, but difficult to find because it is most prevalent in rare earth compounds, which are difficult to isolate elements from. Scandium has very few commercial applications because of the aforementioned facts, and currently its only major application is in aluminium alloys.

Titanium

Titanium (Ti) is an element in period 4, between scandium and vanadium. Titanium is both one of the least dense metals and one of the strongest and most corrosion-resistant, and as such has many applications, especially in alloys with other elements, such as iron. Due to its aforementioned properties, it is commonly used in airplanes, golf clubs, and other objects that must be strong, but lightweight.

Vanadium

Vanadium (V) is an element in period 4, between titanium and chromium. Vanadium is never found in pure form in nature, but is commonly found in compounds. Vanadium is similar to titanium in many ways, such as being very corrosion-resistant, however, unlike titanium, it oxidizes in air even at room temperature. All vanadium compounds have at least some level of toxicity, with some of them being extremely toxic.

Chromium

Chromium (Cr) is an element in period 4, between vanadium and manganese. Chromium is, like titanium and vanadium before it, extremely resistant to corrosion, and is indeed one of the main components of stainless steel. Chromium also has many colorful compounds, and as such is very commonly used in pigments, such as chrome green.

Manganese

Manganese (Mn) is an element in period 4, between chromium and iron. Manganese is often found free in nature, but is also found in combination with iron. Manganese, like chromium before it, is an important component in stainless steel, preventing the iron from rusting. Manganese is also often used in pigments, again like chromium. Manganese is also poisonous; if enough is inhaled, it can cause irreversible neurological damage.

Iron

Iron (Fe) is an element in period 4, between manganese and cobalt. Iron is probably the most well-known element in period 4, being the most common element in the earth and a major component of steel. Iron-56 has the lowest energy density of any isotope of any element, meaning that it is the most massive element that can be produced in supergiant stars. Iron also has some applications in the human body; hemoglobin is partly iron.

Cobalt

Cobalt (Co) is an element in period 4, between iron and nickel. Cobalt is commonly used in pigments, as many compounds of cobalt are blue in color. Cobalt is also a core component of many magnetic and high-strength alloys. The only stable isotope, cobalt-59, is an important component of vitamin B-12, while cobalt-60 is a component of nuclear fallout and can be dangerous in large enough quantities due to its radioactivity.

Nickel

Nickel (Ni) is an element in period 4, between cobalt and copper. Nickel is rare in the earth's crust, mainly due to the fact that it reacts with oxygen in the air, with most of the nickel on earth coming from nickel iron meteorites. However, nickel is incredibly common in the earths core; along with iron it is one of the two main components. Nickel is an important component of stainless steel, and in many superalloys.

Copper

Copper (Cu) is an element in period 4, between nickel and zinc. Copper is one of the few metals that is not white or gray in color, the only others being gold and caesium. Copper has been used by humans for thousands of years to provide a reddish tint to many objects, and is even an essential nutrient to humans, although too much is poisonous. Copper is also commonly used as a wood preservative or fungicides.

Zinc

Zinc (Zn) is an element in period 4, between copper and gallium. Zinc is one of the main components of brass, being used since the 10th century BCE. Zinc is also incredibly important to humans; almost 2 billion people in the world suffer from zinc deficiency. However, too much zinc can cause copper deficiency. Zinc is often used in batteries, aptly named carbon-zinc batteries, and is important in many platings, as zinc is very corrosion resistant.

p-block elements

Gallium

Gallium (Ga) is an element in period 4, between zinc and germanium. Gallium is noteworthy because it has a melting point at about 303 Kelvin, right around room temperature. For example, it will be solid on a typical spring day, but will be liquid on a hot summer day. Gallium is an important component in the alloy galinstan, along with tin. Gallium can also be found in semiconductors.

Germanium

Germanium (Ge) is an element in period 4, between gallium and arsenic. Germanium, like silicon above it, is an important semiconductor and is commonly used in diodes and transistors, often in combination with arsenic. Germanium is fairly rare on earth, leading to its comparatively late discovery. Germanium, in compounds, can sometimes irritate the eyes, skin, or lungs.

Arsenic

Arsenic (As) is an element in period 4, between germanium and selenium. Arsenic, as mentioned above, is often used in semiconductors in alloys with germanium. Arsenic, in pure form and some alloys, is incredibly poisonous to all multicellular life, and as such is a common component in pesticides. Arsenic was also used in some pigments before its toxicity was discovered.

Selenium

Selenium (Se) is an element in period 4, between arsenic and bromine. Selenium is the first nonmetal in period 4, with properties similar to sulfer. Selenium is quite rare in pure form in nature, mostly being found in minerals such as pyrite, and even then it is quite rare. Selenium is necessary for humans in trace amounts, but is toxic in larger quantities.

Bromine

Bromine (Br) is an element in period 4, between selenium and krypton. Bromine is a halogen, never existing in pure form in nature. Bromine is barely liquid at room temperature, boiling at about 330 Kelvin. Bromine is also quite toxic and corrosive, but bromide ions, which are relatively inert, can be found in halite, or table salt. Bromine is often used as a fire retardant because many compounds can be made to release free bromine atoms.

Krypton

Krypton (Kr) is a noble gas, placed under argon and over xenon. Being a noble gas, krypton rarely interacts with itself or other elements; although compounds have been detected, they are all unstable and decay rapidly, and as such, krypton is often used in fluorescent lights. Krypton, like most noble gases, is also used in lighting because of its many spectral lines and the aforementioned reasons.

Biological role

References

↑ "List of Elements of the Periodic Table – Sorted by Abundance in Earth's crust". Science.co.il. Retrieved 2012-08-14.
↑ Gray, Theodore (2009). The Elements: A Visual Exploration of Every Known Atom in the Universe. New York: Black Dog & Leventhal Publishers. ISBN 978-1-57912-814-2.
↑ "Elements in the Modern Periodic Table, Periodic Classification of Elements". Tutorvista.com. Retrieved 2012-08-14.
↑ "It's Elemental – The Element Potassium". Education.jlab.org. Retrieved 2012-08-14.
↑ "Potassium, Chemical Element – Overview, Discovery and naming, Physical properties, Chemical properties, Occurrence in nature, Isotopes". Chemistryexplained.com. Retrieved 2012-08-14.
↑ "Potassium (K) – Chemical properties, Health and Environmental effects". Lenntech.com. Retrieved 2012-08-14.
↑ "Reactions of the Group 2 elements with water". Chemguide.co.uk. Retrieved 2012-08-14.
↑ "Chapter 11. Calcium". Fao.org. Retrieved 2012-08-14.

v t e Periodic tables

Standard form	Periodic table Compact Large f-block in-line, large

Extended form	Extension beyond the 7th period Pyykkö model compact Extended form, large Pyykkö model

Alternative structure	Alternatives Chemical Galaxy Janet table compact

Element properties	Atomic weights Crystal structure Dietary elements Electron affinities Electron configurations Electronegativity by Allen scale Electronegativity by Pauling scale Goldschmidt classification Maximum valences Nutritional elements Platinum group metals (PGM) Rare earth elements Refractory metals

List of elements by	Abundance (in humans) Atomic properties Nuclear stability Production Symbol

Data pages	Abundances Atomic radii Boiling points Critical points Densities Elastic properties Electrical resistivities Electron affinities Electron configurations Electronegativities Hardnesses Heat capacities Heats of fusion Heats of vaporization Ionization energies Melting points Oxidation states Speeds of sound Thermal conductivities Thermal expansion coefficients Vapor pressures

Groups	1 (Alkali metals) 2 (Alkaline earth metals) 3 4 5 6 7 8 9 10 11 12 13 (Boron group) 14 (Carbon group) 15 (Pnictogens) 16 (Chalcogens) 17 (Halogens) 18 (Noble gases)

Metals–nonmetals	Metals Metalloids dividing line Nonmetals Subgroups: Alkali metals Alkaline earth metals Lanthanides Actinides Superactinides Eka-superactinides Transition metals Metalloids Poor metals Polyatomic nonmetals Diatomic nonmetals Noble gases

Blocks	s-block p-block d-block f-block g-block

Periods	1 2 3 4 5 6 7 8 9

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See also	Dmitri Mendeleev Collective names of groups of like elements IUPAC nomenclature systematic element name Trivial name

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