States of Matter and Phase Changes

True (A)

1s2 2s2 2p6 3s2 3p6 4s2 3d4

<p>periods</p> Signup and view all the answers

<p>Group 1/1A = Highly reactive metals that can lose one electron easily Group 2/2A = Reactive metals that usually lose two electrons Group 17/7A = Very reactive nonmetals that gain or share electrons Group 18/8A = Inert gases that do not easily form compounds</p> Signup and view all the answers

<p>Decreases (D)</p> Signup and view all the answers

<p>Calcium</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Barium (C)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>2</p> Signup and view all the answers

<p>Oxygen-18</p> Signup and view all the answers

<p>Chlorine = Gains 1 electron to become Cl- Sulfur = Gains 2 electrons to become S2- Calcium = Loses 2 electrons to become Ca2+ Lithium = Loses 1 electron to become Li+</p> Signup and view all the answers

<p>Mass1 * Abundance1 + Mass2 * Abundance2 (B)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>Cl-</p> Signup and view all the answers

<p>E = hν (B)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>O: with 6 dots around it indicating its 6 valence electrons.</p> Signup and view all the answers

<p>Na3P</p> Signup and view all the answers

<p>Calcium, Bromide = CaBr2 Sodium, Phosphide = Na3P Tin (IV), Sulfide = SnS2 Nickel (III), Selenide = Ni2Se3</p> Signup and view all the answers

<p>Chromium III oxide (A)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>NiPO4</p> Signup and view all the answers

<p>c</p> Signup and view all the answers

A visual representation of electron arrangement in carbon's atomic orbitals showing the filling pattern in its ground state.

The arrangement of electrons in Aluminum's atomic orbitals in the ground state, represented in a sequence of energy levels.

The arrangement of electrons in Chromium's atomic orbitals in the ground state, which deviates from the standard predicted configuration due to electron stability.

The electron configuration corresponds to Magnesium.

A shorthand electron configuration for tin that uses a noble gas core to represent the inner electrons.

A shorthand electron configuration for nickel that uses a noble gas core to represent the inner electrons.

Called periods, they represent increasing levels of electrons surrounding the atomic nucleus.

Called groups or families, they indicate elements with similar chemical properties.

The symbol for Iron is Fe, with an atomic number of 26.

The symbol for Barium is Ba, with an atomic number of 56.

The symbol for Xenon is Xe, with an atomic number of 54.

(mass of isotope 1 × % abundance of isotope 1) + (mass of isotope 2 × % abundance of isotope 2) + ...

A notation for an isotope that indicates the element, mass number, and atomic number.

Sulfur has 6 valence electrons and gains 2 electrons to form an ion, S2-.

Chlorine gains one electron to form an ion, Cl-

Calcium has 2 valence electrons and loses 2 to form ion Ca2+.

E = hν, where E is energy, h is Planck's constant, and ν is frequency.

Planck's constant (h) is measured in joule-seconds (J⋅s).

Frequency (ν) is measured in Hertz (Hz), representing cycles per second.

Use the formula ν= c/λ where c is the speed of light and λ is the wavelength, and c=3.00x10^8 m/s . Plug values into the formula given.

A binary ionic compound is composed of two elements, one metal and one nonmetal, bonded through ionic bonds.

Phosphorus (P) has 5 valence electrons, so its Lewis Dot Structure shows 5 dots around the symbol P.

Magnesium (Mg) has 2 valence electrons, represented by 2 dots around the symbol Mg.

Ternary ionic compounds have three or more elements and contain a polyatomic ion.