What is the formula for percentage of a component in a mixture?

(Mass of Component/ Total Mass of Mixture) x 100

(Total mass of mixture/Mass of component x 100)

(Mass of component/Mass of component x Total Mass of Mixture)

(Mass of component + Total mass of mixture x 100)

How do you find average atomic mass?

Σ (relative abundance of isotope n) × (mass of isotope n)

Σ (mass of isotope - relative abundance)

(mass of isotope / relative abundance) × 100

mass of isotope + relative abundance

Define the structure of an atom.

An atom is structured with a nucleus containing protons and neutrons, surrounded by electrons in orbitals.

Atoms are made up of only protons and electrons.

An atom consists only of electrons without a nucleus.

An atom has a solid core with no empty space around it.

What is the electron configuration order?

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶

1s², 2s², 3s², 2p⁶, 3p⁶, 4p⁶

1s², 2p⁶, 2s², 3d¹⁰, 3s², 4p⁶

1s², 3s², 2p⁶, 2s², 3p⁶, 4p⁶

Define electron configuration.

Electron configuration is when electrons can be thought to exist in "shell" (energy levels) and "subshells" (sublevels).

Electron configuration refers to the energy levels of electrons, which are always filled from highest to lowest.

Electron configuration is the arrangement of protons and neutrons in the nucleus of an atom.

Electron configuration is the process of ionizing an atom by adding or removing electrons to form ions.

What happens to atomic radius across a period (row) using Coulomb's Law?

The atomic radius decreases because of the pull from the nucleus as the outer energy level fills. This causes an increase in charge (negative), which increases the force and makes a smaller radius.

The atomic radius increases because the number of protons and electrons remains constant, and only the distance between them changes.

The atomic radius fluctuates randomly because of varying electron repulsion and random changes in nuclear charge.

The atomic radius remains constant because the number of protons and electrons increases equally, canceling out any changes in radius.

What happens to atomic radius down a group (column) using Coulomb's Law?

The atomic radius increases because of additional energy levels. This increases the distance between electrons and nucleus, causing decrease in force and larger radius.

The atomic radius remains constant because the increasing nuclear charge exactly balances the effect of the additional electron shells.

The atomic radius decreases because the added electron shells decrease the distance between the nucleus and the outermost electrons.

The atomic radius fluctuates irregularly due to varying electron shielding effects and changes in the number of protons.

How do you determine the nearest noble gas?

Find the noble gas (Group 18) atomic number that is closest to the element in the periodic table and has an atomic number less than the element's atomic number.

The nearest noble gas is determined by its color.

The nearest noble gas is based on its reactivity level.

The nearest noble gas is found by its position in the periodic table.

What happens to ionization energy down a group (column) using Coulomb's Law?

Ionization energy decreases down a group because additional electron shells increase the distance from the nucleus, reducing attraction and making electrons easier to remove.

Ionization energy fluctuates unpredictably due to varying electron repulsion and random changes in nuclear charge.

Ionization energy increases because the added electron shells create a stronger attraction between the nucleus and the outermost electrons.

Ionization energy remains constant because the increase in nuclear charge perfectly balances the increased distance from the nucleus.

What happens to ionization energy across a period (row) using Coulomb's Law?

Ionization energy increases because an increasing nuclear charge pulls electrons closer, causing an increase in force and a smaller radius.

Ionization energy decreases because the increasing number of protons reduces the attraction between the nucleus and the electrons.

Ionization energy remains constant because the increase in nuclear charge is balanced by a decrease in the distance between the nucleus and the electrons.

Ionization energy fluctuates due to varying electron repulsion and random changes in nuclear charge.

Define Ionization Energy.

Ionization Energy is the energy required to remove the valence electron from an atom.

Ionization Energy is the energy required to split a molecule into its constituent atoms.

Ionization Energy is the temperature at which an atom becomes ionized.

Ionization Energy is the energy released when an electron is added to a gaseous atom.

Experimental technique used to determine the relative energies of electrons in atoms or ions.

Measures the temperature changes of a sample when exposed to light.

A method for detecting radioactive decay by measuring the energy of emitted particles.

Analyzes the movement of electrons in a magnetic field to determine their energy levels.

Define electronegativity.

Electronegativity is the ability of an atom to attract electrons when bonded.

Electronegativity is the measure of an atom's size.

Electronegativity is the temperature at which a substance changes state.

Electronegativity refers to the energy released during a chemical reaction.

What happens to electronegativity across a period (row) using Coulomb's Law?

Electronegativity increases across a period as the nuclear charge increases, because it wants to fill its shell.

Electronegativity fluctuates across a period due to varying distances between the nucleus and the outermost electrons.

Electronegativity decreases across a period because the additional protons in the nucleus repel electrons, reducing their attraction.

Electronegativity remains constant across a period because the number of electrons and protons increase equally, balancing the attraction.

What happens to electronegativity down a group (column), using Coulomb's Law?

Electronegativity decreases down a group, because there is an increasing distance from the nucleus, causing a decrease in force and a larger radius.

Electronegativity fluctuates down a group due to random changes in the number of protons and electrons.

Electronegativity remains constant down a group because the increase in nuclear charge balances the increased distance from the nucleus.

Electronegativity increases down a group because additional electron shells provide more attraction to bonding electrons.

What columns have the s-block, p-block, and d-block?

s-block: columns 1-2 p-block: columns 13-18 d-block: columns 3-12

s-block: columns 1-3 p-block: columns 10-15 d-block: columns 5-9

s-block: columns 1-4 p-block: columns 12-17 d-block: columns 2-11

s-block: columns 1-2 p-block: columns 14-19 d-block: columns 1-10

Describe how mass spectrometry can be used to determine the isotopic composition of an element.

Mass spectrometry measures the mass-to-charge ratio of ions. It separates isotopes based on their different masses and quantifies their relative abundances.

Mass spectrometry identifies isotopes by observing the color changes of the element when exposed to different wavelengths of light.

Mass spectrometry determines isotopic composition by measuring the temperature of the element and calculating the average mass from that temperature.

Mass spectrometry determines isotopic composition by analyzing the electrical conductivity of the element in a solution.

Explain how successive ionization energies provide evidence for electron configurations.

Successive ionization energies reveal electron configurations by showing where large jumps in energy occur, indicating the removal of electrons from more tightly bound shells.

Successive ionization energies provide evidence for electron configurations by analyzing the temperature changes of the atom when electrons are removed.

Successive ionization energies indicate electron configurations by observing the changes in the atom's volume as electrons are removed.

Successive ionization energies reveal electron configurations by measuring changes in the color of the atom as electrons are removed.

Unit 1 Chemistry Quiz

Authored by Amaya W

Chemistry

10th Grade

NGSS covered

Used 7+ times

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27 questions

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the formula for finding the number of molecules, atoms, or formula units?

Molar mass x Number of molecules

Number of moles / Avogadro's number

Number of moles x Avogadro's number

Avogadro's number / Number of moles

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the formula for finding the number of moles (INCLUDING MASS)?

Volume / Molar mass

Density x Molar mass

Temperature x Molar mass

Mass / Molar mass

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the formula for finding the number of moles (NOT USING MASS) ?

Concentration x Avogadro’s number

Number of atoms/Avogadro’s number

Number of molecules x Avogadro’s number

Temperature/Molar Mass

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What formula is used to find the number of representative particles?

Number of moles x Avogadro’s number

Concentration x Molar mass

Mass/Volume

Molar mass x Number of moles

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the formula for finding mass?

Molar mass x Avogadro’s number

Number of moles × Molar mass

Number of moles x Density

Volume/Concentration

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the formula for finding molar mass (GIVEN ATOMS)?

Density x Volume

∑(Atomic mass of each element x Number of atoms of that element)

Atomic mass of each

element + Number of moles

Number of atoms/Mass of substance

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the formula for finding molar mass (GIVEN MASS OR MOLES)?

Number of moles/Avogadro's Number

Number of moles x Density

Mass/Number of moles

Mass/Concentration

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