chemistry-Periodic table 10

Arrange the following elements from largest to smallest in atomic radii: S, Al, Ar, Si, Mg, P(decreases left-right)

Across period 3: Mg, Al, Si, P, S, Ar

Arrange the following elements from highest to lowest ionization energy: S, Al, Ar, Si, Mg, P(increases left-right)

Ar, S, P, Si, Al, Mg

Which has the larger radius Ar, or Na+?

Argon has a larger radius. They both have the same number of electrons but the sodium ion has one more proton. The sodium ion with 11 protons has a greater pull on the electrons than the 10 protons in argon.

Arrange strontium, beryllium, calcium, and barium in order of decreasing ionization energy. Explain your reasoning using the periodic trends.(decreases from top to bottom

Be, Ca, Sr, Ba

What part of the crust is least dense?

Continental

List the four main layers of the earth.

Crust, mantle, outer core, inner core

When a potassium atom loses one electron to form an K+ ion, the electron is lost from what orbital? Write the electron configuration for this ion. What element has the same electron configuration as the potassium ion?

Electron is lost from the outer 4s orbital Ground State 19K: 1s2 2s22p6 3s23p6 4s1 Ion 19K+ 1s2 2s22p6 3s23p6 The ion has 18 electrons. The Noble gas Ar also has 18 electrons

Name the subatomic particle responsible for chemical reactivity of all elements.

Electrons. (More specifically Valence electrons).

What is the most dense earth layer?

Inner core

Explain the trends for ionization energy, and Electronegativity.

Moving down a group the ionization energy, and electronegativity decrease. Moving from right to left across a period, the ionization energy, and electronegativity also decrease.

What alloy (metals) is found in the inner and outer cores?

Nickel and iron

Explain why the second ionization energy is greater than the first ionization energy in atoms.

Once the first electron is removed, the nucleus draws the electrons closer because the positive nuclear charge is now greater than the total negative electron charge.

Which layer is so hot that the metals are in a liquid state?

Outer core

What name is given to all "A" groups?

Representative elements

Arrange chromium, scandium, cobalt, vanadium in decreasing atomic radius (larger to smaller). Explain your reasoning using the periodic trends.

Sc ,V, Cr, Co,/All the elements across period 4 have a constant energy level and shielding. However, the effective nuclear charge is increasing resulting in greater attractions for the electrons causing electrons to move closer to the nucleus allowing the elements to become smaller in size.

As you travel across period 3 from left to right , explain what causes the radius size to decrease.

Since all the elements are in the same period, energy level and shielding both become constant. The only effect is the effective nuclear charge. As you move from left to right, the effective nuclear charge increases.

define electronegatvity

The ability of an atom to attract electrons to itself.

define ionization

The amount of energy required to completely remove an electron from an atom in the gaseous state.

Explain why the second ionization energy is much greater than the first ionization energy for a sodium atom.

The reasoning is the same as for problem 18. More specifically, the single outer electron in the sodium atom is in the 4th energy level (4s1).

What are the thinnest layer and largest layer of the earth?

Thinnest layer: Crust Largest Layer: Mantle

define periodic law

When elements are listed in order of their atomic numbers, they fall into recurring groups, so that elements with similar properties occur at regular intervals.

The crust is composed of the .......crust and the ___crust.

_continental _ / oceanic

Which outer orbital(s) (sublevel: s, p, d, f) corresponds to the following families: alkaline metals , alkaline Earth Metals, Halogens, Noble Gases transition metals, inner transition metals.

alkaline metals: s1 orbitals alkaline Earth Metals: s2 orbitals Halogens: s2p5 orbitals Noble Gases: s2p6 orbitals transition metals: d orbitals inner transition metals: f orbitals

Elements have similar chemical and physical properties when they are located in the same.....(explain)

group/They all have the same number of valence electrons.

Elements that fill the f orbitals are known as: inner transition metals, metalloids, inner transition metals, halogens.

inner transition metals

The energy needed to remove an electron from a gaseous atom.

ionization energy