A)Metallic bonds are responsible for many properties of metals, such as conductivity. Why is this possible?(1 point)
Responses
An attraction between a positive charge and a negative charge is created.
An attraction between a positive charge and a negative charge is created.
The bonds can shift because valence electrons are held loosely and move freely.
The bonds can shift because valence electrons are held loosely and move freely.
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
Metals have low electronegativity, so they are conductive because they pass charges easily.
Metals have low electronegativity, so they are conductive because they pass charges easily.
Question 2
A)Between which types of elements do ionic bonds occur, and how do electrons act within the bond?(1 point)
Responses
metals and metals, electrons freely moving
metals and metals, electrons freely moving
metals and nonmetals, electrons transferred
metals and nonmetals, electrons transferred
nonmetals and nonmetals, electrons shared
nonmetals and nonmetals, electrons shared
nonmetals and metals, electrons shared
nonmetals and metals, electrons shared
Question 3
A)Which kind of bond would occur between sodium (Na, Group IA) and chlorine (Cl, Group VIIA)?(1 point)
Responses
ionic
ionic
metallic
metallic
no bond
no bond
covalent
covalent
Question 4
A)Which type of bond and how many bonds would occur as carbon dioxide (CO2) is formed from carbon in Group IVA and oxygen in Group VIA?(1 point)
Responses
two ionic bonds
two ionic bonds
one covalent bond
one covalent bond
four covalent bonds
four covalent bonds
three metallic bonds
three metallic bonds
Question 5
A)
Use the periodic table to answer the question.
An illustration shows the periodic table of elements.
The elements in the periodic table are arranged in groups (columns numbered Roman numeral 1 through 18) and periods (rows numbered 1 through 7) such that the atomic number increases along a period from left to right. The elements are divided into the following categories: • Alkali metals • Alkaline earth metals • Transition metals • Post-transition metals • Lanthanoids • Actinoids • Metalloids • Nonmetals • Noble gases • Unknown The elements are also classified on the basis of their physical states at room temperature as follows: • Solid • Liquid • Gas • Unknown The element hydrogen is enlarged with the following properties highlighted. • Chemical symbol: H • Name: Hydrogen • Atomic Number: 1 • Atomic weight: 1.008 Listed by atomic number, symbol, and name. 1, H, Hydrogen. 2, H e, Helium. 3, L i, Lithium. 4, B e, Beryllium. 5, B, Boron. 6, C, Carbon. 7, N, Nitrogen. 8, O, Oxygen. 9, F, Fluorine. 10, N e, Neon. 11, Na, Sodium. 12, M g, Magnesium. 13, A l, Aluminum. 14, S i, Silicon. 15, P, Phosphorus. 16, S, Sulfur. 17, C l, Chlorine. 18, A r, Argon. 19, K, Potassium. 20, C a, Calcium. 21, S c, Scandium. 22, T i, Titanium. 23, V, Vanadium. 24, C r, Chromium. 25, M n, Manganese. 26, F e, Iron. 27, C o, Cobalt. 28, N i, Nickel. 29, C u, Copper. 30, Z n, Zinc. 31, G a, Gallium. 32, G e, Germanium. 33, A s, Arsenic. 34, S e, Selenium. 35, B r, Bromine. 36, K r, Krypton. 37, R b, Rubidium. 38, S r, Strontium. 39, Y, Yttrium. 40, Z r, Zirconium. 41, N b, Niobium. 42, M o, Molybdenum. 43, T c, Technetium. 44, R u, Ruthenium. 45, R h, Rhodium. 46, P d, Palladium. 47, A g, Silver. 48, C d, Cadmium. 49, I n, Indium. 50, S n, Tin. 51, S b, Antimony. 52, T e, Tellurium. 53, I, Iodine. 54, X e, Xenon. 55, C s, Cesium. 56, B a, Barium. 57, L a, Lanthanum. 58, C e, Cerium. 59, P r, Praseodymium. 60, N d, Neodymium. 61, P m, Promethium. 62, S m, Samarium. 63, E u, Europium. 64, G d, Gadolinium. 65, T b, Terbium. 66, D y, Dysprosium. 67, H o, Holmium. 68, E r, Erbium. 69, T m, Thulium. 70, Y b, Ytterbium. 71, L u, Lutetium. 72, H f, Hafnium. 73, T a, Tantalum. 74, W, Tungsten. 75, R e, Rhenium. 76, O s, Osmium. 77, I r, Iridium. 78, P t, Platinum. 79, A u, Gold. 80, H g, Mercury. 81, T L, Thallium. 82, P b, Lead. 83, B i, Bismuth. 84, P o, Polonium. 85, A t, Astatine. 86, R n, Radon. 87, F r, Francium. 88, R a, Radium. 89, A c, Actinium. 90, T h, Thorium. 91, P a, Protactinium. 92, U, Uranium. 93, N p, Neptunium. 94, P u, Plutonium. 95, A m, Americium. 96, C m, Curium. 97, B k, Berkelium. 98, C f, Californium. 99, E s, Einsteinium. 100, F m, Fermium. 101, M d, Mendelevium. 102, N o, Nobelium. 103, L r, Lawrencium. 104, R f, Rutherfordium. 105, D b, Dubnium. 106, Seaborgium, S g. 107, Bohrium, B h. 108, Hs, Hassium. 109, M t, Meitnerium. 110, Darmstadtium, D s. 111, Roentgenium, R g. 112, C n, Copernicum. 113, N h, Nihonium. 114, F l, Flerovium. 115, M c, Moscovium. 116, L v, Livermorium. 117, T s, Tennessine. 118, O g, Oganesson.
According to VSEPR theory, how should the molecular shape of AsF3 be classified?
(1 point)
Responses
tetrahedral, because the arsenic atom forms bonds with the three atoms and the lone pair
tetrahedral, because the arsenic atom forms bonds with the three atoms and the lone pair
trigonal pyramidal, because the arsenic atom forms three single covalent bonds and has one lone pair
trigonal pyramidal, because the arsenic atom forms three single covalent bonds and has one lone pair
trigonal planar, because the arsenic atom forms three single covalent bonds and has no lone pairs
1 answer
Here are the correct responses for each question based on your queries:
Question 1:
B) Metallic bonds are responsible for many properties of metals, such as conductivity. Why is this possible?
Response: The bonds can shift because valence electrons are held loosely and move freely.
Question 2:
B) Between which types of elements do ionic bonds occur, and how do electrons act within the bond?
Response: metals and nonmetals, electrons transferred
Question 3:
C) Which kind of bond would occur between sodium (Na, Group IA) and chlorine (Cl, Group VIIA)?
Response: ionic
Question 4:
D) Which type of bond and how many bonds would occur as carbon dioxide (CO2) is formed from carbon in Group IVA and oxygen in Group VIA?
Response: two covalent bonds
Question 5:
A) According to VSEPR theory, how should the molecular shape of AsF3 be classified?
Response: trigonal pyramidal, because the arsenic atom forms three single covalent bonds and has one lone pair
1 answer