Why is Hydrogen (H) different from other elements in group 1 (alkali metals)?
(1 point)
Responses
[It is the most reactive element in the alkali metals]
[It is the most reactive element in the alkali metals]
[It is a very heavy element, and the alkali metals are relatively light]
[It is a very heavy element, and the alkali metals are relatively light]
[It is not a metal, it is a non-metal]
[It is not a metal, it is a non-metal]
[There are no valence electrons for Hydrogen (H) but the rest of the alkali metals have 1 valence electron.]
[It is not a metal, it is a non-metal]
explain why your right
Hydrogen is different from the other elements in group 1 (alkali metals) because it is not a metal, whereas the rest of the alkali metals are. Metals generally have certain characteristics, such as being shiny, malleable, and good conductors of electricity and heat. On the other hand, hydrogen is a non-metal, which means it lacks these typical metallic properties.
Additionally, the alkali metals in group 1 all have one valence electron in their outermost energy level, while hydrogen does not have any valence electrons. Valence electrons are the outermost electrons of an atom that are involved in chemical reactions. Having one valence electron makes the alkali metals highly reactive.
Therefore, since hydrogen is not a metal and does not have any valence electrons, it is different from the other elements in group 1, which are alkali metals.
Which two statements about metals and non-metals are correct?
(2 points)
Responses
Non-metals can be hammered into thin sheets
Non-metals can be hammered into thin sheets
Metals burn orange
Metals burn orange
Non-metals are brittle
Non-metals are brittle
Metal can be hammered into thin sheets
Two correct statements about metals and non-metals are:
1. Metals can be hammered into thin sheets.
2. Non-metals are brittle.
Which element has two valence electrons?
(1 point)
Responses
Calcium (Ca), Element 20
Calcium (Ca), Element 20
Fluorine (F), Element 9
Fluorine (F), Element 9
Carbon (C), Element 6
Carbon (C), Element 6
Sulfur (S), Element 16
Calcium (Ca), Element 20
Cesium (Cs, Element 55) has LESS valence electrons than Sulfur (S, Element 16).
However, Cesium (Cs) still is a higher energy level than Sulfur (S)?
(1 point)
Responses
True
True
False
AND EXPLAIN WHY YOUR RIGHT
False.
Cesium (Cs) does not have fewer valence electrons than Sulfur (S). Valence electrons are the electrons in the outermost energy level of an atom, and they are responsible for the chemical behavior of an element. Cesium, as an alkali metal in group 1, has only one valence electron. On the other hand, Sulfur, as a non-metal in group 16, has six valence electrons. Therefore, Sulfur has more valence electrons than Cesium.
Additionally, the energy level of an atom is determined by the arrangement of its electrons. In general, as you move down a group on the periodic table, the energy level of the elements increases. Cesium is located in Period 6 and Sulfur is located in Period 3. Since Cesium is in a higher period, it has a higher energy level than Sulfur.
Overall, Cesium has fewer valence electrons but a higher energy level compared to Sulfur. Therefore, the statement "Cesium (Cs) still is a higher energy level than Sulfur (S)" is false.
Explain, in your own words, why Noble Gases (the last family on the periodic table)
are the happiest atoms? In other words, why are they the least reactive elements on the periodic table?
Noble Gases are considered the "happiest" atoms or the least reactive elements on the periodic table because of their stable electron configurations. Atoms are most stable when their valence electron energy levels are full or have achieved a configuration similar to a noble gas.
Noble Gases, such as helium (He), neon (Ne), and argon (Ar), have completely filled valence electron energy levels. This means that their outermost electron shells contain the maximum number of electrons that they can hold. For example, helium has two electrons in its outermost shell, neon has eight, and argon has eight as well. This full valence electron configuration provides a high degree of stability because the electrons are tightly held by the nucleus and there is no strong tendency for these atoms to lose or gain electrons.
Due to their stable electron configurations, Noble Gases do not easily form chemical bonds or react with other elements. Their electron shells are already full, so they do not have a strong desire to gain or lose electrons to achieve a more stable configuration. This makes them inert and less likely to participate in chemical reactions.
Overall, as the Noble Gases have stable, full outer electron configurations, they are considered the happiest atoms and the least reactive elements on the periodic table.
What type of bonding involves the transfer (give and take) of electrons? (1 point)
Responses
This type of bonding does not exist
This type of bonding does not exist
Metallic Bonding
Metallic Bonding
Ionic bonding
Ionic bonding
Covalent Bonding
explain why your right
Ionic bonding involves the transfer (give and take) of electrons.
In ionic bonding, there is a transfer of electrons from one atom to another. This occurs between a metal and a non-metal, or between elements with significantly different electronegativities. The element with a lower electronegativity tends to lose electrons and become a positively-charged ion, called a cation. The element with a higher electronegativity tends to gain these electrons and become a negatively-charged ion, called an anion. The resulting oppositely-charged ions are attracted to each other through electrostatic forces, forming an ionic bond.
The transfer of electrons in ionic bonding allows for the formation of a stable, full outer electron configuration for both participating atoms. This type of bonding is characteristic of many compounds such as salts and binary compounds, where there is a clear transfer of electrons between the elements involved.
Therefore, covalent bonding, on the other hand, involves the sharing of electrons between atoms, not the transfer of electrons.
What type of bonding occurs when electrons are shared (not given or taken)?
(1 point)
Responses
Metallic Bonding
Metallic Bonding
Ionic Bonding
Ionic Bonding
Covalent Bonding
Covalent Bonding
This type of bond does not exist
explain.
Covalent bonding occurs when electrons are shared between atoms.
In covalent bonding, atoms share one or more pairs of electrons in order to achieve a more stable electron configuration. This type of bonding usually occurs between two non-metal atoms with similar electronegativities. Unlike in ionic bonding, where there is a complete transfer of electrons, in covalent bonding, the electrons are shared between the participating atoms.
The shared electrons form a bonding pair, and they are attracted to both nuclei of the participating atoms. This shared electron pair holds the atoms together, creating a covalent bond. The number of shared electron pairs between atoms determines the strength and type of covalent bond, such as single, double, or triple bonds.
Covalent bonding is prevalent in many molecules and compounds found in nature. It forms the basis for the structures and properties of a wide range of substances, from simple diatomic molecules like oxygen (O2), nitrogen (N2) to complex organic compounds like glucose (C6H12O6).
Therefore, when electrons are shared between atoms, it is a characteristic of covalent bonding.
What type of bond is shown in carbon tetrafluoride where Carbon (C) and Fluorine (F) are non-metals?
(1 point)
Responses
Covalent Bonds
Covalent Bonds
Metallic Bonds
Metallic Bonds
Bondo Bonds
Bondo Bonds
Ionic Bonds
EXPLAIN.
The type of bond shown in carbon tetrafluoride (CF4), where carbon (C) and fluorine (F) are non-metals, is a covalent bond.
Carbon tetrafluoride is a molecule composed of one carbon atom and four fluorine atoms. In this compound, carbon and fluorine share electrons to form covalent bonds. Covalent bonds occur when two non-metal atoms share one or more pairs of electrons to achieve a stable electron configuration.
In CF4, each fluorine atom forms a single covalent bond with the central carbon atom. This means that carbon shares one electron with each of the four fluorine atoms, resulting in a total of eight electrons being shared between them. These shared electron pairs create a stable electron arrangement around each atom, fulfilling the octet rule for carbon and the duet rule for fluorine.
Therefore, the bond in carbon tetrafluoride (CF4) is a covalent bond, as it involves the sharing of electrons between the carbon and fluorine atoms, which are both non-metals.