Chemistry Basics Quiz

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

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

<p>1/1800 (D)</p> Signup and view all the answers

<p>12 (A)</p> Signup and view all the answers

<p>Protons have a positive charge, neutrons have no charge. (B)</p> Signup and view all the answers

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

<p>The nucleus is the smallest part of the atom. (C)</p> Signup and view all the answers

<p>PbCl<del>4</del> (D)</p> Signup and view all the answers

<p>Iron(II) fluoride (D)</p> Signup and view all the answers

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

<p>Lead(IV) oxide (D)</p> Signup and view all the answers

<p>Fe^3+^ and O^2-^ (A)</p> Signup and view all the answers

<p>Zinc(II) chloride (B)</p> Signup and view all the answers

<p>Fe(OH)<del>2</del> (A)</p> Signup and view all the answers

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

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

<p>Cu(SO<del>4</del>)<del>2</del> (B)</p> Signup and view all the answers

<p>FeCl<del>3</del> (B)</p> Signup and view all the answers

<p>+4 (D)</p> Signup and view all the answers

<p>FeCl<del>2</del> (A)</p> Signup and view all the answers

<p>Iron(III) sulfide (A)</p> Signup and view all the answers

<p>Lead(II) chloride, PbCl<del>2</del> (B)</p> Signup and view all the answers

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

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

<p>4 (C)</p> Signup and view all the answers

<p>Carbon dioxide, CO2 (A)</p> Signup and view all the answers

<p>The atom that can form the greatest number of covalent bonds (C)</p> Signup and view all the answers

<p>6 (B)</p> Signup and view all the answers

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

<p>8 (D)</p> Signup and view all the answers

<p>1 (C)</p> Signup and view all the answers

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

<p>Electrostatic attraction between positive and negative ions (C)</p> Signup and view all the answers

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

<p>Iron(III) sulfate (D)</p> Signup and view all the answers

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

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

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

<p>The number of valence electrons increases by one for each subsequent group. (C)</p> Signup and view all the answers

<p>They do not exceed two electrons in the first shell. (A)</p> Signup and view all the answers

<p>They are located in the nucleus at the center. (D)</p> Signup and view all the answers

<p>They occupy defined orbits at fixed distances from the nucleus. (A)</p> Signup and view all the answers

<p>Electrons fill from the lowest energy shell to the highest. (D)</p> Signup and view all the answers

<p>Electrons have no defined location and float aimlessly. (A)</p> Signup and view all the answers

<p>Atoms with similar electron configurations often have similar chemical properties. (B)</p> Signup and view all the answers

<p>The maximum capacity of electron shells. (B)</p> Signup and view all the answers

<p>The electrostatic forces between oppositely charged ions are very strong. (B)</p> Signup and view all the answers

<p>It consists of a regular three-dimensional network of positive and negative ions. (B)</p> Signup and view all the answers

<p>The arrangement of ions causes them to shatter easily under external force. (D)</p> Signup and view all the answers

<p>When molten or dissolved in water. (B)</p> Signup and view all the answers

<p>They are mostly soluble in water. (D)</p> Signup and view all the answers

<p>Molecules have a finite number of atoms of each type in a definite structure. (B)</p> Signup and view all the answers

<p>Ionic bonds from electrostatic forces. (B)</p> Signup and view all the answers

<p>There is no fixed number of ions, leading to a network structure. (D)</p> Signup and view all the answers

A polyatomic ion with the formula OH⁻, consisting of one oxygen and one hydrogen atom.

A polyatomic ion with the formula SO₄²⁻, consisting of one sulfur and four oxygen atoms.

A polyatomic ion with the formula CO₃²⁻, consisting of one carbon and three oxygen atoms.

A polyatomic ion with the formula HCO₃⁻, contains a hydrogen ion with carbonate.

A polyatomic ion with the formula NO₃⁻, consisting of one nitrogen and three oxygen atoms.

A polyatomic ion with the formula PO₄³⁻, consists of one phosphorus and four oxygen atoms.

A polyatomic ion with the formula C₂H₃O₂⁻, associated with vinegar.

A polyatomic ion with the formula NH₄⁺, composed of nitrogen and hydrogen.

Arrangement of positive and negative ions in a 3D network.

Attractive forces between oppositely charged ions, forming ionic bonds.

The bond formed due to electrostatic attraction between ions.

Ionic compounds have high melting points due to strong ionic bonds.

Ionic compounds break easily when force is applied due to their rigid structure.

Ionic compounds conduct electricity when molten or dissolved in water.

Ionic compounds are mostly soluble in water and can dissociate into ions.

Ionic compounds are not defined as molecules because they lack a fixed number of ions.

Electrons in the outermost shell of an atom that can participate in chemical bonding.

The vertical columns in the periodic table that indicate the number of valence electrons in elements.

The distribution of electrons in an atom's electron shells and subshells.

The central part of an atom, containing protons and neutrons.

Regions surrounding the nucleus where electrons are found.

Positively charged particles found in the nucleus of an atom.

Neutral particles in the nucleus that contribute to atomic mass.

The first 20 elements in the periodic table, which are easier to work with for drawing configurations.

A bond formed by sharing pairs of electrons between atoms.

A diagram that shows the bonding between atoms using dots for electrons.

Sum of valence electrons from all atoms in a molecule.

The atom that can form the most bonds is placed in the center.

A bond created by sharing one pair of electrons.

Bonds formed by sharing two or three pairs of electrons, respectively.

1. Draw atoms, 2. Count electrons, 3. Identify central atom, 4. Distribute electrons, 5. Draw bonds.

Elements that only form ions with a 2+ charge.

Metals that can form ions with multiple stable charges.

A stable ion of copper with a +1 charge.

A stable ion of copper with a +2 charge.

An ion that only forms Zn2+ with a +2 charge.

An ion that only forms Ag+ with a +1 charge.

The naming convention includes the metal name and charge as a Roman numeral.

Compound formed from Cu+ and Cl-, represented as CuCl.

Compound formed from Cu2+ and Cl-, represented as CuCl2.

Compound formed from Fe3+ and O2-, indicated as Fe2O3.

The electrostatic attraction between positive and negative ions.

Compound formed from Pb4+ and Cl-, represented as PbCl4.

Compound with the formula ZnS, formed by Zn2+ and S2-.

Compound with Ag+ and I-, represented as AgI.

The number of protons in the nucleus of an atom, determining the element.

Negatively charged particles orbiting the nucleus of an atom.

Atoms of the same element with different numbers of neutrons, thus varying mass numbers.

Properties and reactions of an element, influenced by its electron configuration.

Total number of protons and neutrons in an atomic nucleus.

The charge of a particle compared to other particles; protons are +1, electrons are -1, neutrons are 0.