IB SL Chemistry Test 3 revision on topics 2, 3 and briefly 4 | Baamboozle - Baamboozle

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You may use your electronegativity values in Section 8 of the IB data booklet, determine the bonding in methane (CH4)

an example of non-polar covalent bonding

an example of ionic bonding

an example of hydrogen bonding

an example of polar covalent bonding

Which electron transition emits radiation of the longest wavelength?

A

B

C

D

Which electron configuration is correct for the selenide ion, Se2−?

1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p4

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

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

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4

Which of the following atoms would have the largest second ionization energy?

Na

S

Cl

Mg

Formula of nitrate

NO3-

What elements have zero electronegativity?

noble gases

Choose from the following (see image)

c

b

d

a

What is the product of Cl2(g) + KI(aq) --> ?

Cl2(g) + 2KI(aq) --> I2 (s) + 2KCl(aq)

Order the elements S, Cl, and F in terms of increasing atomic radii.

S, F, Cl

S, Cl, F

F, Cl, S

Cl, F, S

Which element is this: [Kr]5s1 4d10

Ag (silver)

formula of sulphate ion

SO4^2-

Which is the electron configuration of a chromium atom in the ground state?

[Ne]3s2 3p6 4s1 3d4

[Ar ]3d3

1s2 2s2 2p6 3s2 3p6 4s2 3d4

[Ar]4s1 3d5

The amount of energy released when an electron is added to a neutral atom to form a negative ion

atomic radii

ionization energy

electronegativity

electron affinity

List the following atoms in order of increasing ionization energy: Li, Na, C, O, F.

Na < Li < C < O < F

The __________ electrons are in the outermost principal quantum level of an atom

valence

Chemical formula for copper (I) sulfate

Cu2SO4

Which of the following will have similar properties to 1s2 2s2 2p6 3s2 3p2?

oxygen

carbon

phosphorus

chlorine

Which element is isoelectronic with argon?

F-

S2-

Rb+

Mg2+

Which group does bromine belong to? (name of group)

halogen

Which group does potassium belong to? (name of group)

alkali metals

Which property increases down Group 1, the alkali metals?

atomic radius

ionization energy

electronegativity

electron affinity

Describe the structure and bonding in solid magnesium oxide.

a giant ionic lattice with electrostatic attraction between oppositely charged ions

Formulate an equation for the reaction of magnesium oxide with water.

MgO(s) + H2O(l) --> Mg(OH)2

Common name for a hydrogen atom that contains a neutron

deuterium

tritium

helium

protium

The four lines observed in the visible emission spectrum of hydrogen tell us that:

Only certain energies are allowed for the electron in a hydr

The hydrogen molecules they came from have the formula H4.

The spectrum is continuous.

There are four electrons in an excited hydrogen atom.

Which of the following frequencies corresponds to light with the longest wavelength?

8.50 × 1020 s–1

4.12 × 105 s–1

3.00 × 1013 s–1

9.12 × 1012 s–1

Which electron transition in the hydrogen atom emission spectrum emits radiation with the longest wavelength?

n = 1 → n = 2

. n = 2 → n = 1

n = 4 → n = 1

n = 3 → n = 2

How many protons, neutrons and electrons?

20 protons, 21 neutrons, 18 electrons

Ethanoic or acetic acid, CH3COOH, is a weak acid that is often used in the creation of vinegar.Note the two distinctly different bonds between carbon (C) and oxygen (O). Which option contains the correct information of these bonds?

option B

option A

option C

option D

Of the following elements, which has the lowest first ionization energy?

Ba

Cl

Ca

Si

State and explain the trend in first ionization energy values across the period Li to F.

IE increases across period due to increased attraction between p+ in nucleus and valence e-.

Which of the following is the most electronegative element?

N

K

P

O

Chemical formula for sodium oxide

Na2O

Which form of electromagnetic radiation has the longest wavelengths?

MICROWAVES

GAMMA RAYS

RADIO

INFRARED

How many electrons in a Cl- ion?

16

35

36

18

What is the condensed electron configuration of the Fe2+ ion?

[Ar]3d6

Which of the following shows the proper condensed electron configuration of a copper atom (Cu)?

[Ar] 3d¹⁰ 4s¹

1s2 2s2 2p6 3s2 3p6 3d10 4s

[Ar] 4s2 3d9

1s2 2s2 2p6 3s2 3p6 4s2 3d9

How many unpaired electrons does chlorine have in its ground state?

[Ne]3s23p5 so just ONE (1)

Which oxide, when added to water, produces the solution with the highest pH?

CO2

SO3

Na2O

BeO

List the following atoms in order of increasing ionization energy: Li, Na, C, O, F.

O<F<C<Li<Na

Na<Li<C<O<F

F<O<C<Li<Na

Li<Na<C<O<F

Choose the element with the highest ionization energy.

Mg

P

Al

Na

2. Which is correct for the following regions of the electromagnetic spectrum?

B

A

C

D

7. What is the formula for an ionic compound formed by element X (Group 3) and element Y (Group 6 / 16)?

XY2

X3Y2

X2Y3

XY3

How many valence electrons does an element with atomic number 19 have?

1

7

2

8

Which of these periodic trends is a man-made number?

electron affinity

electronegativity

ionization energy

molecular mass

For the set of elements Li, O, Ne, and Na, which element has the largest atomic radius?

Ne

O

Na

Li

In general, the ionization energy and electron affinity involve more energy from __________ (left to right or right to left) in a period of the periodic table. Why?

The increase is from left to right because of the increase in nuclear charge.

What is the product of I2(g) + KBr(aq) --> ?

No reaction because bromine is more reactive

IB SL Chemistry Test 3 revision on topics 2, 3 a ...