Atomic Masses and Ionic Compounds

<p>One-twelfth the mass of a carbon-12 atom. (C)</p> Signup and view all the answers

<p>140.28 u (B)</p> Signup and view all the answers

<p>Because most elements exist as mixtures of isotopes with different masses. (D)</p> Signup and view all the answers

<p>102.13 u (A)</p> Signup and view all the answers

<p>10.8 u (A)</p> Signup and view all the answers

<p>626.28 u (B)</p> Signup and view all the answers

<p>18.02 u (C)</p> Signup and view all the answers

<p>120.37 u (C)</p> Signup and view all the answers

<p>Atomic masses are average masses based on the isotopic composition of an element. (B)</p> Signup and view all the answers

<p>179.89 u (A)</p> Signup and view all the answers

<p>6.941 u (C)</p> Signup and view all the answers

<p>64.06 u (D)</p> Signup and view all the answers

<p>The average mass of all the isotopes of the element. (D)</p> Signup and view all the answers

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

<p>The desire to be in a lower energy state (C)</p> Signup and view all the answers

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

<p>Transfer of electrons from one atom to another (C)</p> Signup and view all the answers

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

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

<p>The distribution of electrons in different energy levels (C)</p> Signup and view all the answers

<p>It becomes positively charged (D)</p> Signup and view all the answers

<p>Sodium chloride (NaCl) (D)</p> Signup and view all the answers

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

<p>Sharing of electrons between atoms (C)</p> Signup and view all the answers

A unit that describes the masses of individual atoms and molecules, defined as one-twelfth of the mass of a carbon-12 atom.

Proton: 1.00728 u, Neutron: 1.00866 u, Electron: 0.000549 u.

Atomic mass is the weighted average of isotopes, while mass number is the total count of protons and neutrons in an atom.

Atoms of the same element with different masses due to varying numbers of neutrons.

Calculates atomic mass as the average mass of isotopes, based on their abundance.

For Boron, atomic mass is 10.8 u based on isotopes 20% Boron-10 and 80% Boron-11.

The total mass of a molecule calculated by summing the atomic masses of its constituent atoms.

For N2O3, molecular mass is 76.001 u based on 2 Nitrogens and 3 Oxygens, calculated from the periodic table.

Average weight of an element's isotopes, weighted by their natural abundance.

Total count of protons and neutrons in an atomic nucleus.

Groups of two or more atoms bonded together, forming the smallest unit of a compound.

Number of protons in the nucleus of an atom, defining the element.

One or two-letter abbreviations representing an element on the periodic table.

Compounds formed from the electrostatic attraction between oppositely charged ions.

Electrically charged particles formed when atoms gain or lose electrons.

Ions with a positive charge, formed by losing electrons.

Ions with a negative charge, formed by gaining electrons.

Atoms tend to gain, lose, or share electrons to have eight in their outer shell.

Transfer of electrons between two atoms to achieve octets.

Sharing of electrons between two atoms.

Cations are named by adding the word 'ion' after the element name.

Anions are named using the stem of the element with an -ide suffix.

The arrangement of electrons in an atom's electron shells.