HSPS Standard 1 Test 2025 2026

The neutral atom model would have 11 protons and 11 electrons; the ion model would have 11 protons and 10 electrons.

The neutral atom would have 11 protons and 10 electrons; the ion would have 11 protons and 11 electrons.

The neutral atom would have 10 protons and 11 electrons; the ion would have 11 protons and 11 electrons.

The neutral atom would have 11 protons and 12 electrons; the ion would have 11 protons and 10 electrons.

They are different elements because they have different numbers of subatomic particles.

They are the same element but different isotopes because they have different neutron counts.

They are ions of the same element because they have different numbers of neutrons.

They are the same element with identical properties because they have equal protons and electrons.

The ion has 17 protons, 18 neutrons, and 16 electrons with a total mass of 35 amu.

The ion has 17 protons, 18 neutrons, and 18 electrons with a total mass of 35 amu.

The ion has 17 protons, 17 neutrons, and 18 electrons with a total mass of 36 amu.

The ion has 16 protons, 18 neutrons, and 18 electrons with a total mass of 35 amu.

X and Y are isotopes; Z is an ion of the same element as X and Y.

X and Z are isotopes; Y is an ion of the same element as X and Z.

Y and Z are isotopes; X is an ion of the same element as Y and Z.

All three particles are ions of different elements with similar properties.

W and X are isotopes of the same ion; Y is a neutral atom; Z is an ion of a different element.

W and Y are different ions of the same element; X and Z are neutral atoms of different elements.

W, X, and Y are all related to the same element; Z represents a completely different element.

All four particles represent neutral atoms of different elements with varying mass numbers.

All elements in Period 3 are gases at room temperature due to their similar atomic sizes.

Elements on the left side are solids, while elements on the right side include gases.

All elements in Period 3 are solids at room temperature due to strong metallic bonding.

Elements alternate between solid and gas phases in a regular pattern across the period.

The number of valence electrons decreases from 8 to 1 as atoms become more metallic.

The number of valence electrons increases from 1 to 8 then drops to 0 for the noble gas.

The number of valence electrons increases from 1 to 8 as atoms become more nonmetallic.

The number of valence electrons remains constant at 8 for all elements in the period.

Element A, because it forms a positive ion and is solid at room temperature.

Element B, because it has properties between metals and nonmetals in this period.

Element C, because it changes from solid to gas state easily.

This table contains only metals and nonmetals, with no metalloids present.

Elements form ions to achieve the same electron configuration as the nearest transition metal.

Elements form ions to achieve the electron configuration of the nearest noble gas.

Elements form ions to minimize the repulsion between their valence electrons.

Elements form ions to maximize the attraction between positive and negative charges.

Metallic character decreases across the period, with a sharp transition from metals to nonmetals.

Metallic character decreases across the period, with metalloids showing intermediate properties.

All elements in the same period have similar properties regardless of their position.

Nonmetallic character is strongest at the beginning of the period and weakest at the end.

Element W will have 7 valence electrons and tend to form W⁻ ions.

Element W will have 17 valence electrons and form W¹⁷⁺ ions.

Element W will have 8 valence electrons and not form ions.

Element W will have 7 valence electrons and form W⁷⁺ ions.

Y will be a metal, solid at room temperature, with 6 valence electrons, forming Y⁶⁺ ions.

Y will be a nonmetal, solid at room temperature, with 6 valence electrons, forming Y²⁻ ions.

Y will be a metalloid, liquid at room temperature, with 16 valence electrons, forming Y⁴⁻ ions.

Y will be a nonmetal, gas at room temperature, with 3 valence electrons, forming Y³⁻ ions.

Element Z will have more valence electrons than nitrogen and be more metallic.

Element Z will have the same number of valence electrons as nitrogen and be more metallic.

Element Z will have fewer valence electrons than nitrogen and be less metallic.

Element Z will have the same number of valence electrons as nitrogen and be less metallic.

Predictions 1 and 2 only, because they are based on group trends.

Predictions 1, 2, and 3 only, because they follow group characteristics.

All four predictions, because they all follow established periodic trends.

Predictions 1, 2, and 4 only, because Group 17 elements show these patterns.

R will be a nonmetal with 7 valence electrons, forming R⁻ ions, and be less reactive than fluorine.

R will be a metal with 4 valence electrons, forming R⁴⁺ ions, and have properties similar to tin.

R will be a metalloid with 17 valence electrons, forming R¹⁷⁻ ions, and be more reactive than iodine.

R will be a nonmetal with 6 valence electrons, forming R²⁻ ions, and have properties between sulfur and selenium.