Interpretation: The reason for placement of argon before potassium in spite of its greater atomic mass and the
Concept Introduction:
Periodic Table: The available chemical elements are arranged considering their
In periodic table the horizontal rows are called periods and the vertical column are called group.
In periodic table the horizontal rows are called periods and the vertical column are called group. There are seven periods and 18 groups present in the table and some of those groups are given particular name as follows,
Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the
Atomic mass: It is generally expressed in terms of atomic mass unit
Mass number: It is given by the total number of protons and the neutrons present in the nucleus of the element and it is denoted by symbol A. The subscript that lies on the left side of the symbol of the element represents the mass number.
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Chemistry: Atoms First
- (a) Would you expect scandium oxide to be a solid, liquid, or gas at room temperature?arrow_forwardUntil the early 1960s the group 8A elements were called the inert gases; before that they were called the rare gases. The term rare gases was dropped after it was discovered that argon accounts for roughly 1% of Earth’s atmosphere. (a) Why was the term inert gases dropped? (b) What discovery triggered this change in name? (c)What name is applied to the group now?arrow_forwardBoron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forward
- Arrange in order of increasing nonmetallic character. (a) the period 4 elements Ga, Ge, Ti (b) the Group 5A elements P, Bi, and Narrow_forward25) Which of the following elements has the highest ionization energy? Ca Al Ne Ba Clarrow_forwardHow many inner, outer, and valence electrons are present in an atom of each of the following elements? (a) Br (b) Cs (c) Cr (d) Sr (e) Farrow_forward
- Arrange in order of increasing nonmetallic character. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 4 elements V, Ge, and K (b) the Group 5A elements N, As, and Bi Arrange in order of increasing atomic size. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 3 elements Mg, Si, and Ar (b) the Group 2A elements Ca, Ba, and Srarrow_forwardGIVEN: (Probable atomic weights: N=14; O=16) Physical properties Nitrous oxide Nitrogen dioxide Nitric oxide Density (kg/m³) Boiling point (°C) Freezing point (°C) Enthalpy of vaporization (kJ/mol) Enthalpy of fusion (kJ/mol) 1.98 88.48 2.05 1.34 21 152 164 90.86 - 11.2 16.53 32 13.83 82.05 33.18 90.25 Your answer What is the most applicable state of matter for the given compounds in the table? * Liquid Liquid Crystal Solid Gas Which has the lowest molecular weight among the three compounds? Your answer here will be the basis for answering the next items below. * Nitric oxide Nitrogen dioxide Nitrous oxide O O Oarrow_forwardhelp with only 6d 6e and 6f please!arrow_forward
- Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forwardGiven the following reactions: (I) M + Cl2 --> MCl2; (II) M + O2 --> MO2 (III) 4M + O2 --> 2M2O; (IV) 6M + N2 --> 2M3N In which of the above reaction(s) could M represent a Group IA element? (A) III only (B) II and III (C) II, III, and IV (D) All of themarrow_forwardUntil the early 1960s, the group 8A elements were calledthe inert gases. (a) Why was the term inert gases dropped?(b) What discovery triggered this change in name? (c) Whatname is applied to the group now?arrow_forward
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