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True. In a metal lattice, electrons are not bound to individual atoms and can move freely throughout the structure. This mobility of electrons is what allows metals to conduct electricity and heat efficiently. The presence of a sea of delocalized electrons contributes to the characteristic properties of metals, such as their malleability and ductility.
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True or false the bonds within a metal lattice are weak?
False. The bonds within a metal lattice are typically strong due to the metallic bonding, which involves the attraction between positively charged metal ions and a "sea" of delocalized electrons. This strong bonding contributes to the unique properties of metals, such as conductivity and malleability.
Is it true or false that the properties of a solid metal can be explained by the structure of been bonding among the metal atoms?
True. The properties of a solid metal, such as conductivity, malleability, and ductility, can be explained by the metallic bonding among metal atoms. In metallic bonds, electrons are delocalized, allowing them to move freely throughout the metal lattice, which contributes to these characteristic properties. This unique bonding structure distinguishes metals from other types of materials.
Oxidation involves the gain of electrons for a substance. true or false?
False. Oxidation involves the loss of electrons for a substance.
When elections are transferred between two atoms a covalent bond is formed true or false?
This is false. Transfer of electrons produces an ionic bond.
True or false an impurity raises the melting point of an organic compound?
False. In general, impurities lower the melting point of an organic compound by disrupting the crystal lattice structure.
Is it true or false metallic bonds are formed from the sharing of valence electrons?
False. Metallic bonds are formed by the delocalization of electrons throughout a lattice structure of metal atoms. Valence electrons are not shared between specific pairs of atoms like in covalent bonds, but rather move freely throughout the metal structure.
Is it true or false that the properties of a solid metal can be explained by the structure of been bonding among the metal atoms?
True. The properties of a solid metal, such as conductivity, malleability, and ductility, can be explained by the metallic bonding among metal atoms. In metallic bonds, electrons are delocalized, allowing them to move freely throughout the metal lattice, which contributes to these characteristic properties. This unique bonding structure distinguishes metals from other types of materials.
Oxidation involves the gain of electrons for a substance. true or false?
False. Oxidation involves the loss of electrons for a substance.
Reduction is the gain of oxygen by a metal true or false?
False
An ionic compound is made of a nonmetal and a metal true or false?
True. Ionic compounds form between a metal and a nonmetal. The metal loses electrons to become a cation (positively charged ion), while the nonmetal gains these electrons to become an anion (negatively charged ion).
True or false Covalent bonds can best be describe as a swapping of electrons?
False. Covalent bonds involve the sharing of electrons between atoms, not the swapping of electrons.
Is the properties of a metal are related to bonds true or false?
true.
Is it true or false every element has the same valence?
False. Elements have different numbers of valence electrons, which determines their reactivity and chemical properties. The valence electrons are the electrons in the outermost energy level of an atom.
When elections are transferred between two atoms a covalent bond is formed true or false?
This is false. Transfer of electrons produces an ionic bond.
The loss of electrons from food molecules is reduction true or false?
It is false that the loss of electrons from food molecules is reduction. Electrons are negatively charged subatomic particles.
Is the reactivity of the metal elements generally increase as you move from left to right across the periodic table true or false?
True. Generally, the reactivity of metal elements increases as you move from left to right across the periodic table. This is because as you move towards the right, the elements have fewer electrons in their outer shell, making them more likely to lose electrons and react with other elements.
Is it true or false that the crystal lattice of ionic compounds affects their melting and boiling points?
True. The crystal lattice structure of ionic compounds plays a significant role in determining their melting and boiling points. The stronger the forces holding the ions in the lattice together, the higher the melting and boiling points of the compound.
