{"id":170,"date":"2018-03-20T20:17:35","date_gmt":"2018-03-21T00:17:35","guid":{"rendered":"https:\/\/opentextbc.ca\/physicalgeologyh5p\/chapter\/5-2-bonding-and-lattices-2\/"},"modified":"2023-07-04T12:47:07","modified_gmt":"2023-07-04T16:47:07","slug":"bonding-and-lattices","status":"publish","type":"chapter","link":"https:\/\/opentextbc.ca\/physicalgeologyh5p\/chapter\/bonding-and-lattices\/","title":{"raw":"5.2 Bonding and Lattices","rendered":"5.2 Bonding and Lattices"},"content":{"raw":"Atoms seek to have a full outer shell. For hydrogen and helium, a full outer shell means two electrons. For other elements, it means 8 electrons. Filling the outer shell is accomplished by transferring or sharing electrons with other atoms in chemical bonds.\u00a0 The type of chemical bond is important for the study of minerals because the type of bond will determine many of a mineral's physical and chemical properties.\r\n

Ionic Bonds<\/h1>\r\nConsider the example of halite again, which is made up of sodium (Na) and chlorine (Cl).\u00a0 Na has 11 electrons: two in the first shell, eight in the second, and one in the third (Figure 5.7, top). Na readily gives up the third shell electron so it can have the second shell with 8 electrons as its outermost shell.\u00a0 When it loses the electron, the total charge from the electrons is -10, but the total charge from the protons is +11, so it is left with a +1 charge over all.\r\n\r\n[caption id=\"attachment_164\" align=\"aligncenter\" width=\"400\"]\"\" Figure 5.7<\/strong> Electron configuration of sodium and chlorine atoms (top). Sodium gives up an electron to become a cation (bottom left) and chlorine accepts an electron to become an anion (bottom right). Source: Steven Earle (2015), CC BY 4.0. Image source.<\/a>[\/caption]\r\n\r\nChlorine has 17 electrons: two in the first shell, eight in the second, and seven in the third. Cl readily accepts an eighth electron to fill its third shell, and therefore becomes negatively charged because it has a total charge of -18 from electrons, and a total charge of +17 from protons.\r\n\r\nIn changing their number of electrons, these atoms become ions<\/strong>\u2014the sodium loses an electron to become a positive ion or cation<\/strong>,[footnote]You can remember that a cation is positive by remembering that a cat has paws (paws sounds like \"pos\" in \"positive\"). You could also think of the \"t\" in \"cation\" as a plus sign.[\/footnote] and the chlorine gains an electron to become a negative ion or anion<\/strong> (Figure 5.7, bottom). Because negative and positive charges attract, sodium and chlorine ions stick together, creating an ionic bond<\/strong>. In an ionic bond, electrons can be thought of as having transferred from one atom to another.\r\n
\r\n\r\nCation or Anion?<\/strong>\r\n\r\n[h5p id=\"54\"]\r\n\r\n<\/div>\r\n

Covalent Bonds<\/h1>\r\nSome elements can also form bonds by sharing electrons rather than giving away or receiving them. This will happen when electrons are held especially tightly by their atoms. Chlorine gas (Cl2<\/sub>, Figure 5.9) is formed when chlorine atoms share two outer-shell electrons so that each has a complete outer shell. This is called a covalent bond<\/strong>.\r\n\r\n[caption id=\"attachment_165\" align=\"aligncenter\" width=\"400\"]\"\" Figure 5.9<\/strong> A covalent bond between two chlorine atoms. The electrons are black in the left atom, and blue in the right atom. Two electrons are shared (one black and one blue) so that each atom appears to have a full outer shell. Source: Steven Earle (2015), CC BY 4.0. Image source.<\/a>[\/caption]\r\n\r\nCarbon is another atom that participates in covalent bonding.\u00a0 An uncharged carbon atom has six protons and six electrons. Two of the electrons are in the inner shell and four are in the outer shell (Figure 5.10, left). Carbon would need to gain or lose four electrons to have a filled outer shell, and this would create too great a charge imbalance. Instead, carbon atoms share electrons to create covalent bonds (Figure 5.10, right).\r\n\r\n[caption id=\"attachment_166\" align=\"aligncenter\" width=\"434\"]\"\" Figure 5.10<\/strong> The electron configuration of carbon (left) and the sharing of electrons in covalent C bonding (right). The electrons shown in blue are shared between adjacent C atoms. Source: Steven Earle (2015), CC BY 4.0. Image source.<\/a>[\/caption]\r\n\r\nIn the mineral diamond (Figure 5.11, left), carbon atoms are linked in a three-dimensional framework, where each carbon atom is bonded to four other carbon atoms. Every bond is a very strong covalent bond.\r\n\r\n[caption id=\"attachment_167\" align=\"aligncenter\" width=\"450\"]\"\" Figure 5.11<\/strong> Covalently bonded structures. Left: Diamond with three-dimensional structure of covalently bonded carbon. Right: Graphite with covalently bonded sheets of carbon. Sheets are held together by weaker van der Waals forces. Source: Karla Panchuk (2018), CC BY 4.0. Modified after Materialscientist (2009), CC BY-SA 3.0. Image source.<\/a>[\/caption]\r\n

Other Types of Bonds<\/h1>\r\nMost minerals are characterized by ionic bonds, covalent bonds, or a combination of the two, but there are other types of bonds that are important in minerals.\r\n

Van der Waals Forces and Hydrogen Bonds<\/h2>\r\nConsider the mineral graphite (Figure 5.11, right): carbon atoms are linked together in sheets or layers in which each carbon atom is covalently bonded to three others. Graphite-based compounds are strong because of the covalent bonding between carbon atoms within each layer, which is why they're used in high-end sports equipment such as ultralight racing bicycles. Graphite itself is soft, however, because the layers themselves are held together by relatively weak Van der Waals forces<\/strong>.\r\n\r\nVan der Waals forces, like hydrogen bonds<\/strong>, work because molecules can be electrostatically neutral, but still have an end that is slightly more positive and an end that is slightly more negative. In water molecules (Figure 5.12, left), the bent shape puts the hydrogen atoms on one side of the molecule, and the oxygen atom, with more electrons, on the other. The charge is distributed asymmetrically across the water molecule. Contrast this with the straight carbon dioxide molecule (Figure 5.12, right). The slightly more negative oxygen atoms on the ends are distributed symmetrically on either side of the carbon atom.\r\n\r\n[caption id=\"attachment_168\" align=\"aligncenter\" width=\"500\"]\"\" Figure 5.12<\/strong> Hydrogen bonding. Water molecules (left) are polar molecules (their charge is distributed asymmetrically). Slightly negative parts of the molecule are attracted to slightly positive parts of other water molecules. Carbon dioxide (right) is a non-polar molecule. The slightly negative oxygen atoms are distributed symmetrically on either side of the carbon atom. Source: Karla Panchuk (2018), CC BY-SA 4.0. Modified after Querter (2011, CC BY-SA 3.0; view source<\/a>) and Jynto (2011, CC0 1.0; view source).<\/a>[\/caption]\r\n

Metallic Bonds<\/h2>\r\nMetallic bonding<\/strong> occurs in metallic elements because they have outer electrons that are relatively loosely held. (The metals are highlighted on the periodic table in Appendix 1<\/a>.) When bonds between such atoms are formed, the dissociated electrons<\/strong> can move freely from one atom to another. This feature accounts for two very important properties of metals: their electrical conductivity and their malleability (they can be deformed and shaped).\r\n\r\n[caption id=\"attachment_169\" align=\"aligncenter\" width=\"475\"]\"\" Figure 5.13<\/strong> Metallic bonding. Dissociated electrons (grey dots) move between metal atoms. Source: Karla Panchuk (2018), CC BY-SA 4.0. Nucleus by Fornax (2010), CC BY-SA 3.0. Image source.<\/a>[\/caption]\r\n\r\n
\r\n\r\nChemical Bond Types<\/strong>\r\n\r\n\r\n
\r\n\r\nFill in the missing words to complete the definitions of the different types of chemical bonds.<\/strong>\r\n\r\nIn\u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/span> bonding, atoms share electrons. Diamond, one of the hardest naturally occurring substances, is formed from this type of bond.\r\n\r\n \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/span> bonding is what allows copper to be drawn into a wire instead of breaking.\r\n\r\nHalide elements, such as chlorine, which have space for one additional electron in their outer shells, will undergo \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/span> bonding with elements like sodium than have an electron to give up.\r\n\r\nWhen weak \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/span> bonds connect strongly bonded layers, the mineral will come apart in sheets.\r\n\r\nTo check your answers, navigate to the below link to view the interactive version of this activity.<\/strong>\r\n\r\n<\/div>\r\n[h5p id=\"55\"]\r\n<\/div>","rendered":"

Atoms seek to have a full outer shell. For hydrogen and helium, a full outer shell means two electrons. For other elements, it means 8 electrons. Filling the outer shell is accomplished by transferring or sharing electrons with other atoms in chemical bonds.\u00a0 The type of chemical bond is important for the study of minerals because the type of bond will determine many of a mineral’s physical and chemical properties.<\/p>\n

Ionic Bonds<\/h1>\n

Consider the example of halite again, which is made up of sodium (Na) and chlorine (Cl).\u00a0 Na has 11 electrons: two in the first shell, eight in the second, and one in the third (Figure 5.7, top). Na readily gives up the third shell electron so it can have the second shell with 8 electrons as its outermost shell.\u00a0 When it loses the electron, the total charge from the electrons is -10, but the total charge from the protons is +11, so it is left with a +1 charge over all.<\/p>\n

\"\"
Figure 5.7<\/strong> Electron configuration of sodium and chlorine atoms (top). Sodium gives up an electron to become a cation (bottom left) and chlorine accepts an electron to become an anion (bottom right). Source: Steven Earle (2015), CC BY 4.0. Image source.<\/a><\/figcaption><\/figure>\n

Chlorine has 17 electrons: two in the first shell, eight in the second, and seven in the third. Cl readily accepts an eighth electron to fill its third shell, and therefore becomes negatively charged because it has a total charge of -18 from electrons, and a total charge of +17 from protons.<\/p>\n

In changing their number of electrons, these atoms become ions<\/strong>\u2014the sodium loses an electron to become a positive ion or cation<\/strong>,[1]<\/sup><\/a> and the chlorine gains an electron to become a negative ion or anion<\/strong> (Figure 5.7, bottom). Because negative and positive charges attract, sodium and chlorine ions stick together, creating an ionic bond<\/strong>. In an ionic bond, electrons can be thought of as having transferred from one atom to another.<\/p>\n

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Cation or Anion?<\/strong><\/p>\n

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