Chemistry Chapter 2 Quiz

Atoms are the smallest unit of an element that retains the chemical properties of that element. They are made up of even smaller particles called protons, neutrons, and electrons.

Atoms of different elements have a different number of protons in their nucleus. This difference in proton number gives each element its unique properties.

Electrons are negatively charged particles that orbit the nucleus of an atom in a cloud-like region called the electron shell.

The atomic number (Z) of an element is the number of protons found in the nucleus of an atom of that element. It's a unique identifier for each element.

The atomic number determines the identity of an element. It also tells us the number of electrons in a neutral atom.

The mass number (A) of an atom is the total number of protons and neutrons in its nucleus. It represents the atom's approximate atomic mass.

Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. This results in different atomic masses.

The average mass number of an element, calculated by averaging the masses of its isotopes.

When determining the number of neutrons, round the atomic mass to the nearest whole number. Numbers 0-4 round down, and 5-9 round up.

Atoms of the same element that have the same number of protons but different numbers of neutrons.

The total number of protons and neutrons in an atom's nucleus.

The overall charge of an atom is neutral (0). This is because the number of positively charged protons equals the number of negatively charged electrons.

The number of protons in an atom's nucleus.

A neutral atom has the same number of electrons as protons.

Subatomic particles found in the nucleus of an atom. They have no charge.

Subtract the atomic number (number of protons) from the mass number (protons + neutrons) to find the number of neutrons in an atom.

A pure substance that cannot be broken down into simpler substances by ordinary chemical means. It contains only one type of atom.

The smallest particle of an element that retains the chemical properties of that element.

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

Protons determine the element's identity.

The total number of protons and neutrons in the nucleus of an atom.

The average mass of an atom of an element, taking into account the different isotopes.

The number of neutrons in an atom can be calculated by subtracting the atomic number from the mass number.

A chart that organizes the elements by increasing atomic number, highlighting their repeating properties.

Horizontal rows in the periodic table that represent elements with the same number of electron shells.

Highly reactive metals located in Group 1 of the periodic table. Their reactivity increases as you move down the group, making them more reactive with increasing atomic number.

Alkaline earth metals are found in Group 2 of the periodic table. They are less reactive than alkali metals but still react with oxygen and water under the right conditions.

Highly reactive non-metals located in Group 17 of the periodic table. They exist in different states at room temperature: fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.

Alkaline earth metals are less reactive than alkali metals. Alkali metals are more reactive because they have only one valence electron, making them more likely to lose it and form a positive ion.

The most stable and unreactive elements found in Group 18 of the periodic table. They are colorless gases at room temperature and used in lights to produce different colors.

Elements that are typically shiny, malleable, ductile, good conductors of heat and electricity, and often magnetic.

Elements that are generally dull, poor conductors of heat and electricity, non-malleable, non-ductile, and not magnetic. They can exist as solids, liquids, or gases at room temperature.

Elements that share properties of both metals and non-metals. They are often semiconductors, meaning they can conduct electricity under certain conditions.

Most metals are solid at room temperature, with the exception of mercury, which is a liquid.

Most metalloids are solid at room temperature.

Non-metals can exist as solids, liquids, or gases at room temperature.

Metals are typically shiny and have a metallic luster, giving them a bright and reflective appearance.

Non-metals are typically dull and lack a metallic luster. They can have a variety of colors, but are often not reflective like metals.

Metals are ductile, meaning they can be drawn into wires, and malleable, meaning they can be hammered into thin sheets.

Non-metals are not ductile or malleable, meaning they can't be drawn into wires or hammered into sheets.