Objective Questions

Example: Li, Na, K, and Rb all have one __________ electron.

Across a period, each element differs by the addition of one __________ and one…

Example: The electron configurations change from Li ([He]2s¹) to Be ([He]2s²) t…

__________ refers to recurring trends in element properties.

These trends are caused by predictable variations in element __________.

Periodic properties depend on an element's __________ configuration.

Examples include atomic radius, ionic radius, ionization energy, electron affin…

Atomic radius is defined as half the distance between two nuclei of a _________…

The general trend is that atomic radius __________ across a period.

Atomic radius decreases across a period due to an increase in __________ charge.

Added electrons are pulled more strongly as protons increase, a concept called …

The first factor is the __________ level of the valence electron; higher levels…

The second factor is __________ charge; a higher charge pulls electrons closer.

The third factor is the __________ effect; inner electrons shield outer electro…

Ionization Energy (IE) is the energy required to remove the most __________ bou…

The process of removing an electron is always __________ (absorbs energy).

The energy to remove the *first* electron is called the __________ Ionization E…

Ionization energy and atomic radius are __________ proportional.

The __________ the atom, the easier it is to remove an electron (lower IE).

IE increases with higher __________ charge.

IE decreases with greater shielding effect and larger atomic __________.

Removing an electron from a __________ or half-full sublevel requires extra ene…

Full (e.g., ns², np⁶) and half-full (e.g., np³) orbitals are particularly _____…

Elements with these configurations have __________ ionization energies than exp…

Down a group, first ionization energy __________.

This is because atomic radius increases and the __________ effect increases.

Across a period, ionization energy generally __________ from left to right.

Exceptions to this trend occur at __________ and half-full orbitals.

There is a large jump in ionization energy when removing an electron from a fil…

Valence electrons do not __________ each other effectively, so effective nuclea…

First ionization energies decrease __________ a group.

The element with the *lowest* ionization energy is in the __________ corner of …

The element with the *highest* ionization energy is in the __________ corner (e…

Ionization energies increase diagonally from lower left to __________.

Electronegativity is a measure of an atom's ability to attract __________ in a …

The concept was pioneered by __________.

__________ have low electronegativity (tend to release electrons).

__________ have high electronegativity (tend to attract electrons).

__________ atoms are more electronegative than large ones.

A large difference in electronegativity between two atoms leads to a bond with …

Electronegativity __________ down a group because atomic size increases and shi…

Electronegativity __________ across a period from left to right.

The most electronegative element is __________.

Elements of the same group have the same number of __________ electrons. (Q1)

Elements are arranged in order of increasing __________. (Q2)

Among Li, Mg, Na, and Al, the element with the *lowest* first IE is __________.…

Atomic size decreases across a period due to an increase in the nuclear force o…

Given electron configurations [He]2s¹, [Ne]3s¹, and [Ar]4s¹, the order of *incr…

Metals have __________ ionization energy because their valence electrons are fa…

The correct order for first ionization energies among Be, B, N, and O is ______…

The number of protons in an atom determines its:

The energy flowing through the boundary as a result of temperature difference is

Science is not

The family name of Group VII elements is

The number of electrons in the outmost shell of group 16 elements?

The general trend down the groups of the periodic table is?

Which of the following is not a scientific theory?

Naturally occurring silicon is a mixture of 92.23 % silicon-28, 4.67 % of silic…

Which substance in 1 mol dm⁻³ aqueous solution would have the same hydrogen ion…

3.0 g of NH₃ reacts with 5.5 g of O₂ to form NO and H₂O. Which reactant is the …

In the reaction C₆H₆ + Br₂ → C₆H₅Br + HBr, 30.0 g benzene reacts with 65.0 g br…

70 g MnO₂ reacts with 3.5 moles of HCl according to MnO₂ + 4HCl → MnCl₂ + Cl₂ +…

257.8 mL of 0.0468 M Pb(NO₃)₂ is mixed with 156.00 mL of 0.095 M Na₂S. What mas…

0.886 moles of NO reacts with 0.505 moles of O₂ according to 2NO + O₂ → 2NO₂. H…

Magnesium reacts with iron(III) oxide: 3Mg + Fe₂O₃ → 3MgO + 2Fe. If 1.00 mol Mg…

Using the reaction 3Mg + Fe₂O₃ → 3MgO + 2Fe, what maximum mass of Fe can be pro…

What mass of ZnCl₂ forms when 3.27 g Zn reacts with 3.30 g HCl? Reaction: Zn + …

In MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O, how many moles of HCl react with 1 mole of…

In 2NO + O₂ → 2NO₂, what is the mole ratio of NO to O₂?

What is the coefficient of the chemical equation given below? ?C₈H₁₈(l) + ?O₂ →…

In the reaction C₆H₆ + Br₂ → C₆H₅Br + HBr, what is the mole ratio between benze…

Which substance in 1 mol dm⁻³ aqueous solution would have the same hydrogen ion…

Consider the equation 2C₄H₁₀ → 2SO₂(g) + 18H₂O(l). The number of moles of CO₂ p…

When 3.0g of NH₃ reacts with 5.5g of O₂ to produce NO and H₂O, determine the li…

Benzene reacts with bromine to produce bromobenzene and hydrobromic acid. If 30…

70 grams of manganese dioxide is mixed with 3.5 moles of hydrochloric acid. How…

If 257.8 mL of a 0.0468 M solution of lead nitrate is added to 156.00 mL of a 0…

In an experiment, 0.886 moles of NO is mixed with 0.505 moles of O₂. Calculate …

You are provided with 1.00 mol of Mg and 0.252 mol of iron (III) oxide. The bal…

You are provided with 1.00 mol of Mg and 0.252 mol of iron (III) oxide. The bal…

What mass of ZnCl₂ can be prepared from the reaction of 3.27 g of zinc with 3.3…

The mass (in grams) of FeSO₄·7H₂O required for preparation of 125 mL of 0.90 M …

Calculate the mass percent of bromine in C₂H₃BrF₂. (C=12, H=1, Br=80, F=19)

In which type of mixture are the components uniformly distributed and not visib…

Calculate the mass percent of iodine in C₂H₃IF₂. (C=12, H=1, I=127, F=19)

A 0.01 M solution of a weak monoprotic acid has a pH of 4.50. What is the Ka of…

What is the mass percent of bromine in C₂H₃BrF₂? (C=12, H=1, Br=80, F=19) (Dupl…

The compound CH₃CH₂CH=CH₂ reacts with HBr to give primarily:

What is the mass percent of chlorine in C₂H₃ClF₂? (C=12, H=1, Cl=35.5, F=19) (D…

A 0.025 M solution of a weak monoprotic acid has a pH of 3.80. Calculate the Ka…

For the equilibrium: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g); ΔH = -198 kJ mol⁻¹. Which of th…

Which three subatomic particles make up atoms?

What is a molecule?

Which of the following is a common molecule?

Which of the following is true about molecules and compounds?

What are cations?

What are anions?

For metallic cations in Groups I, II, and III, what do their charges correspond…

What is atomicity?

What is the atomicity of noble gases like He, Ne, and Ar?